Important Announcements Important Announcements Chemistry Ch-1 Basic Concepts Welcome To Your Quiz "Ch-1 Basic Concepts" Click on "Start Quiz" To Continue... 1. The smallest particle which can take part in a chemical reaction ? Ion Molecule Neutron Atom None 2. Which of the following is a molecule ? H He Na K None 3. Haemoglobin is made up of how many molecules ? 9000 10,000 12.000 15,000 None 4. The soul chemistry is its dealing with ? Internal Structure Compsition Properties of Matter Composition & Properties of Matter None 5. If an atom loses three electron such as "Al" how many positive charge will it gain ? 1 2 3 4 None 6. Empirical formula or formula unit of a compound ? May Be Similar or Different Always Same Always Different None None 7. The mass of One Mole of Water is ? 8 g 12 g 16 g 18 g None 8. Which of the following is a substance ? Sea Water Brass Tap Water Graphite None 9. Electrometer is also called ? Voltmeter Ion Collector Ampere Meter Galvanometer None 10. The volume occupied by 1.4 g of N2 at S.T.P is ? 2.24 dm^3 22.4 dm^3 1.12 dm^3 112 dm^3 None 11. Percentage of oxygen in water is ? 80% 88.89% 8.8% 9.8% None 12. Molecular mass of CaCO3 is ? 100 120 130 140 None 13. Carbon has Isotopes ? 1 2 3 4 None 14. Tin has Isotopes ? 7 9 11 12 None 15. Simplest formula that gives the small whole number ratio between the atoms of different elements ? Mole Number Molecular Formula Empirical Formula Ionic Formula None 16. Molecular Formula = n x moles n x empirical formula n x mass None None 17. Isotopes are sister atoms of same element with similar chemical properties but different ? Atomic Number Atomic Weight Atomic Mass Atomic Volume None 18. Atoms of which one of the following element have independent existence ? F Cl Kr N None 19. Which of the following element can exist in monoatomic form ? Oxygen Nitrogen Chlorine Helium None 20. Moles = Mass/Molar Mass Mass Molar Mass None None 21. One of the substances is used to absorb CO2 gas in combustion analysis which is that substancе ? 50% KOH Al2O3 Mg(CIO4)2 SiO2 None 22. Avogadro's Number = ? 6.02 x 10^23 6.02 x 10^22 6.002 x 10^23 6 x 10^23 None 23. In Mass-Mass relationship we can find the mass of a 1 substance with the help of ______ other substance ? Mass Volume Molar Mass None None 24. The mass of one mole of electrons is ? 1.008 mg 0.55 mg 0.055 mg 1.0 mg None 25. 27g of Al will react completely with how much mass of O2 to produce AL2O3 ? 30 g of O 25 g of O 32 g of O 24 g of O None 26. The largest number of molecules are present in ? 3.6 g of H2O 4.8 g of C2H5OH 2.8 g of CO None None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-2 Experimental Techniques In Chemistry Welcome To Your Quiz "Ch-2 Experimental Techniques In Chemistry" Click on "Start Quiz" To Continue... 1. Which one of the following substance is used as decolorizing agent: Animal Charcoal Conc. H₂SO₄ CaCl₂ Silica Gel None 2. Direct conversion of solid into vapours is called: Crystallization Sublimation Distribution Vaporization None 3. Which chemical do not undergo sublimation: KMnO₄ NH₄Cl Nephthaline Iodine None 4. The most common solvent used in solvent extraction is: Acetone Ethanol Rectified Spirit Diethyl Ether None 5. In paper chromatography the mobile phase is usually: Liquid Ammonia Water Organic Liquid None of these None 6. The iodine present in the water can be separated by which of the following techniques: Sublimation Chromatography Filtration Solvent Extraction None 7. Repeated extraction using small portion of solvent are more: Accurate Efficient Slow Rapid None 8. Purity of substance is checked by: Sublimation Chromatography Filtration Solvent Extraction None 9. In CCl₄ Solvent, I₂ Shows: Blue colour Pink colour Purple colour Brown colour None 10. When hot saturated solution is coold very slowly we get: Medium size crystals Large size crystals Premature crystals No crystals None 11. Solvent extraction is an equilibrium process and it's controlled by: Law of mass action Distribution law The amount of solvent used The amount of salute None 12. Insoluble particles can be separated from a liquid by: Sublimation Chromatography Filtration Solvent Extraction None 13. The comparative rates at which the salute moves in the paper chromatography depend on: Size of paper Rf values of solutes Temperature of experiment Size of the chromatography tank used None 14. Solvent extraction method is a particularly useful technique for separation when the product to be separated is: Non-volatile or thermally unstable Volatile or thermally unstable Volatile or thermally stable None of these None 15. The solid which is left over the filter paper is called: Filtrate Residue Crystals Mud None 16. Safe and most reliable method of drying crystal is through: Filter paper Desiccator Oven None None 17. The solution left behind after the filtration of crystals is called: Residue Mud Crystals Mother Liquor None 18. Size of filter paper is selected according to the amount of: Solution Precipitate Water Solid particles None 19. Which of the following cannot be filtered by sintered glass crucible: KMnO₄ solution Concentrated HCl Concentrated HF AgCl precipitates None 20. Sintered crucible is made up of: Plastic Glass Porcelain Steal None 21. Gooch crucibles are made up of: Plastic Glass Porcelain Steal None 22. Cold finger is used for effective: Filtration Sublimation Crystallization Chromatography None 23. The solvent or mixture of solvent used for the separation of compound is called: Mobile phase Mixed phase Stationary phase Solid phase None 24. Mixture of NaCl and NH₄Cl can be separated by: Filtration Sublimation Crystallization Chromatography None 25. The component which shows maximum affinity for stationery phase will have: Large Rf Value Small Rf Value Intermediate Rf Value None None 26. The separation of two miscible liquid by heating due to difference of their boiling point is called: Vaporization Distillation Condensation Sublimation None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-3 Gases Welcome To Your Quiz "Ch-3 Gases" Click on "Start Quiz" To Continue... 1. Partial pressure of oxygen in human lungs in torr is: 161 116 159 760 None 2. If absolute temperature of a gas is doubled and pressure is reduced to one half, the volume of the gas will: Remain unchanged Increase four times Reduce to 1/4 Be doubled None 3. The molar volume of CO2 is maximum at: S.T.P 127°C and 1 atm 0°C and 2 atm 273K None 4. Which gas has highest diffusion rate? SO2 Cl2 NH3 CO2 None 5. Which one of the following molecules have maximum root mean square velocity at 25°C: CO2 H2S NH3 CO None 6. The ideal gas constant R, when expressed in dm³ atm. mol-¹.K-¹ units have a value of: 0.0821 1.0821 82.21 82.1 None 7. Which of the following will have the same number of moles at S.T.Р? 280 cm³ of CO2 and 280 cm³ of N2O 11.2 dm³ of O2 and 32 g of 02 44 g CO2 and 11.2 dm³ of CO 28.0g N2 and 5.6 g O2 of oxygen None 8. Pilots feel uncomfortable breathing in unpressurized cabins: Due to high pressure of CО2 Due to low pressure of O2 Due to fatigue Due to low pressure of CO2 None 9. If the values of 'a' and 'b' in Van der Waal's equation are close to zero for a gas, then the gas is: Ideal Non-ideal highly polar Liquefied easily None 10. Which of the following is not an intermolecular force between molecules: Covalent bonds Hydrogen bonds De-bye forces Ion dipole forces None 11. Equal masses of methane and oxygen are mixed in an empty container at 25°С. The fraction of total pressure exerted by oxygen is: 1/3 8/9 1/9 16/17 None 12. The value of R (in Nm K-¹ mol-¹) is: 8.214 8.314 0.0321 62.4 None 13. The order of rate of diffusion of gases NH3, SO2, Cl2 and CO2 is: NH3 > SO2 > Cl2 > CO2 NH3 > CO2 > SO2 > Cl2 Cl2 > SO2 > CO2 > NHз NH3 > CO2 > Cl2 > SO2 None 14. One torr is equal to: One atmosphere One Pascal One mm of Hg 76 cm of Hg None 15. Which gas deviate more from ideal behaviour at high pressure: H2 He Ar NH3 None 16. THe kinetic molecular theory of gases was put forward in 1738 by: Boltzman Maxwell Clausius Bernouli None 17. 0.5 mole of NO2 and 0.5 mole of SO3 gas have equal: Volume Molecules Mass Atoms None 18. Which gas cannot be dried by passing over H2SO4: SO2 H2 NO2 H2S None 19. Which one of the following has least critical temperature: O2 NH3 H2O HCl None 20. Lind's method is employed for: Separation of gases Expansion of gases Compression of gases Liquifaction of gases None 21. Pressure remaining constant, at which temperature the volume of a gas will become twice of what it is at 0°C: 546°C 200°C 546K 273K None 22. Plasmas are found in everything from sun to: Atoms Molecules Electrons Quarks None 23. The density of a gas can be determined by formula: d = PM/RT d = RT/PM d = PMR/T d = PMT/R None 24. The absolute zero is: Attainable May be attainable Un attainable in gaseous state May not be attainable None 25. Calorie is equivalent to: 0.4184 J 41.84 J 4.184 J 10.418 J None 26. Absolute zero is equal to: 273°C -273°C 0°C 273 K None 27. Standard temperature: 0°C 75°C 273°C 100°C None 28. Which pair of gases do not obey Dalton's law of partial pressure: H2 and O2 N2 and O2 NH3 and HCl H2 and He None 29. For a gas obeying Boyle's law if pressure is doubled the volume becomes: Double Half 2 Times 1/2 None 30. Mathematically Boyle's law is shown as: PT = K VT = K P/T =K PV = K None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-4 Liquids & Solids Welcome To Your Quiz "Ch-4 Liquids & Solids" Click on "Start Quiz" To Continue... 1. The boiling point of the halogens: Increase down the group Decrease down the group Remains constant can't be predicted None 2. A crystal system in which all the axes and angles are unequal is called: Tetragonal system Monoclinic system Triclinic system Cubic system None 3. Water may boil at 120°C when external pressure is: 369 torr 700 torr 760 torr 1489 torr None 4. Transition temperature of tin is: 95.5°C 13.2°C 0°С 128.5°C None 5. Hydrogen bonding is strongest in: HI HBr HCI HF None 6. London dispersion forces are significant for: Polar molecules Ionic solids Metals Non polar molecules None 7. The boiling points of higher alkanes are greater than those of lower alkanes due to the reasons that: Higher alkanes have greater number of atoms The polarizability of higher alkanes is greater Higher alkanes have zigzag structures Higher alkanes have greater hydrogen bonding None 8. K2SO4 and K2CrO4 are isomorphic solids and exist in: Cubic form Orthorhombic form Trigonal form Tetragonal None 9. The forces which are present between the ions and the water molecules are known as: Dipole induced forces Ion-dipole forces Dipole-dipole forces London dispersion forces None 10. Liquids evaporate at every temperature. When the temperature becomes constant for a liquid then: Rate of evaporation is greater than the rate of condensation. The rate of condensation is greater than the rate of evaporation. The rate of condensation and evaporation becomes equal Depends upon the nature of the liquid None 11. The size of diameter of double helix of DNA is: 18-20 Å 20-30 Å 1-10 Å 25-30 Å None 12. Polarizability is measure of extent of distortion: Qualitative Quantitative Systematic None of these None 13. The number of Cl ions per unit cell of NaCl is: 8 6 4 2 None 14. Allotropy is the property of: Compound Element Atoms Mixture None 15. Which one is the following is a pseudo solid: CaF2 NaCl Borax Glass None 16. The structure of sodium chloride is: Body centered cube Face centered cube Simple cube None None 17. Polarizability generally ________ down the group: Increases Decreases Negligible Remain Constant None 18. Bucky balls is an allotropic form of: Sulphur Carbon Silica Tin None 19. Liquid hydrocarbon is: Methane Propane Ethane Hexane None 20. Heat change for one mole of a solid during converting into liquid is called: Molar heat of vaporization Molar heat of sublimation Molar heat of fusion Enthalpy change None 21. Ionic solid don't conduct the electrical current because: Ions do not have translatory motion Free electrons are less The coordination number of the ion is very high Strong covalent bonds are present in their structure None 22. The number of Na+ ions which surround each Cl ion in the NaCI crystal is: 4 6 8 12 None 23. Vapour pressure is not affected by: Surface area Temperature Pressure Intermolecular forces None 24. Kerosene oil is used to kill mosquitoes because it has surface tension: Very strong Very weak Zero No effect on surface tension None 25. The existence of an element in more than one crystalline forms: Allotropy Isotropy Isomorphism Polymorphism None 26. Glycerine decomposes at its: Melting point Boiling point Freezing point Critical point None 27. Crystal system shown by diamond is: Cubic Tetragonal Monoclinic Hexagonal None 28. Which of the following does not form a molecular crystal? Ice Graphite Iodine Sugar None 29. Water has maximum density at: 4°C 0°C 100°C 10°C None 30. Which substance shows anisotropic behavior in electrical conductivity? Diamond Graphite KCI Ice None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-5 Atomic Structure Welcome To Your Quiz "Ch-5 Atomic Structure" Click on "Start Quiz" To Continue... 1. An orbital can accommodate maximum electrons: 10 14 6 2 None 2. Lyman Series is obtained when electron in an atom jumps from higher energy level to: Ground level 2nd level 3rd level 4th level None 3. When 6d orbital is complete, the entering electron goes into: 7f 7s 7p 7d None 4. Lyman series occur in: Visible region U.V. region I.R. region None of these None 5. e/m value for positive rays is maximum for: Hydrogen Helium Oxygen Nitrogen None 6. According to Bohr's atomic model, radius of second orbit of hydrogen atom is: 0.529 Å 2.116 Å 4.0 Å 5.0 Å None 7. The limiting line of Balmer series lies in the region: Visible U.V. Near I.R Far I.R None 8. Free neutron decays into a proton with the emission of an electron and a_______: Positron Neutrino Beta Particle Helium nucleus None 9. Bohr's model of atom is contradicted by: Photo electric effect Heisenberg's uncertainty principle Pauli's exclusion principle A Aufbau principle None 10. What is the value of (n + l) for the 3s sub-shell? 2 1 5 3 None 11. K-series X-Rays have wavelength: Longer Smaller Same Different None 12. Mass of one mole of electron is: 0.55 mg 0.184 mg 1.673 mg 1.008 mg None 13. For the P sub shell the azimuthal quantum number "l"is: 2 3 0 1 None 14. When the Azimuthal quantum number is 3 then 'm' can have: 5 values 7 values 2 values 3 values None 15. If an electron is free from the attraction of nucleus then its energy is: Negative Positive Zero None of these None 16. Which one of the following series lies in ultraviolet region: Lyman Balmer Paschen Brackett None 17. The d-subshell consists of: 5-orbitals 6-orbitals 7-orbitals 10-orbitals None 18. Lines of Paschen series are produced when electrons jump from higher orbits to --------- orbit. 1st 2nd 3rd 4th None 19. The electronic configuration of an atom is 1s2,2s2,2p4. The number of unpaired electrons in this atom is: 0 2 4 6 None 20. An orbital which is spherical and symmetrical is: s-orbital p-orbital d-orbital f-orbital None 21. Bambardment of a-particles on Beryllium (Be) atom, emits neutron and this process is called: Natural radioactivity Artificial radioactivity Pauli's exclusion principle Hund's rule None 22. Splitting of spectral lines when atoms are subjected to strong magnetic field is called: Zeeman effect Stark effect Compton effect Photoelectric effect None 23. In discharge tube experiment, the pressure of gas was maintained at: 760 torr 0.001 torr 0.01 torr 10 torr None 24. When 4s orbital is complete, the electron goes into: 4p 3d 4f None 25. The electrons occupying an orbital are distinguished by: Magnetic quantum number Principal quantum number Azimuthal quantum number Spin quantum number None 26. Total number of spectral regions in sunlight spectrum is: 4 6 7 8 None 27. The mass of proton is (in kg): +1.6 x 10-19 -1.6 x 10-19 1.672 x 10-27 9.1 x 10-31 None 28. Balmer series in hydrogen spectrum lies in the region: Ultraviolet Visible Infrared Microwave None 29. Angstrom is the unit of: time length mass frequency None 30. Negative charge on cathode rays we established by: William Crook J. Perrin R.A Millikan Hittrof None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-6 Chemical Bonding Welcome To Your Quiz "Ch-6 Chemical Bonding" Click on "Start Quiz" To Continue... 1. Which of the following molecules has a coordinate covalent bond? HСІ NaCl NH4CI AICI3 None 2. Ionic compounds are mostly obtained by the combination of group: 3 and 5 2 and 5 4 and 8 1 and 7 None 3. In sp² hybridization, the orbitals are oriented at an angle of: 109.5° 120° 180° 0° None 4. Which of the following species has unpaired electron in anti bonding molecular orbitals? H2 He2 02+2 N₂-2 None 5. Carbon dioxide and methane have dipole moment value: Zero and 1.85. D( 1.70 D and 1.80 D Both have zero None of these None 6. Оctet rule is not followed in the formation of: NF3 CF4 CCl4 PCl5 None 7. Total number of bonds in C2H4 molecule is: 6 2 8 4 None 8. Ionic, covalent and co-ordinate covalent bond are present in: SO2 NH4CI C2H2 H2O None 9. Bond angle between H-S-H bonds is: 105.5° 107.5° 92° 95° None 10. The number of electrons shared in SF6: 4 12 6 8 None 11. Which of hydrogen halides has highest % of ionic character? HCl HBr HF HI None 12. The geometry of ethane is: Tetrahedral Trigonal planar Linear V-shaped None 13. The paramagnetic property of oxygen is well-explained on the basis of: VSEPR theory VB theory MO theory None of these None 14. The bond order of N2 according to MO theory is: 0 1 2 3 None 15. The molecule which can not form co-ordinate covalent bond with H+ ion is: NH3 H20 PH3 CH4 None 16. Which of the following species has configuration of Neon? Na+ Ca+2 CI-1 None of these None 17. M.O.T was proposed by: Moseley Werner Kossel Mullikan None 18. The number of bonds in Nitrogen molecule is: One sigma and one Pi One sigma and two Pi Three sigma only Two sigma and one Pi None 19. O2 molecule is paramagnetic because: Bonding electrons are equal to the anti-bonding electrons Bonding electrons are more than anti-bonding electrons Bonding electrons are less than anti-bonding electron It contains unpaired electrons None 20. NH3 has a net dipole moment, but BF3 has zero dipole movement because: B is less electronegative than N F is more electronegative than N BF3 is pyramidal while NH3 is planar NH3 is pyramidal while BF3 is trigonal planar None 21. The bond energy of hydrogen molecule is KJ/mole: 436 440 420 460 None 22. The value of dipole moment of CS2 is: 0.12D 0D 1.61D 0.95D None 23. The elements having low ionization energy are: Non-metal Metals Semi-metal Metalloids None 24. Which of the following is not isoelectronic with rest of the threе? K+ Na+ Cl- S-2 None 25. Total number of sigma bonds in Ethyne (CH=CH) are: 5 3 2 4 None 26. Formation of chemical bond takes place when: Energy is absorbed Forces of repulsion overcome forces of attraction Forces of attraction are equal to forces of repulsion Forces of attraction overcome forces of repulsion None 27. The shielding effect is responsible for: The decrease in nuclear attractive influence over the valence electrons The increase in nuclear attractive influence over the valence electrons The decrease repulsion between nucleus and inner electrons The increase in attraction between nucleus and inner electrons. None 28. The nature of bond in diamond is: Electrovalent Covalent Metallic Co-ordinate covalent None 29. Maximum electronegativity is of: N F O Cl None 30. Which of the hydrogen halides has the highest percentage of acid character: HCl HBr HF HI None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-7 Thermochemistry Welcome To Your Quiz "Ch-7 Thermochemistry" Click on "Start Quiz" To Continue... 1. Spontaneous reactions are: Reversible Irreversible Non irreversible None of these None 2. The standard heat changes occur at: 25°C and 2 atm 298 K and 1 atm 25°C and 1 mm hg 273 K and 1 atm None 3. H+ + OH- → H20 the change in enthalpy for reaction is called: Heat of reaction heat of formation Heat of neutralization Heat of combustion None 4. The enthalpy change when one mole of substance is completely burnt in excess of oxygen is called: Enthalpy of atomization Enthalpy of neutralization Enthalpy of Combustion Enthalpy of formation None 5. Enthalpy change for the reaction: CH4(g) + 202(g)→CO2(g) + 2H2O(l) is called enthalpy of: Formation Combustion Neutralization Atomization None 6. Standard enthalpies are measured at: 273 K 298K 373 K All of these None 7. The exothermic process is: Evaporation Sublimation Respiration Boiling None 8. A state function which describes together the internal energy and the product of volume is called: Enthalpy Internal energy Work Free energy None 9. Whenever a reaction is exothermic, then it means that: The heat is transferred from surroundings to the system The heat content of the reactant is greater than product The heat content of the reactants is less than those of products The heat is transferred from system to the surroundings. None 10. In a Bomb calorimeter, the reaction are carried out at constant: Pressure work volume None of these None 11. Whenever a reaction is endothermic, than it means that: Heat is transferred from surrounding to the system Heat is transferred from system to the surrounding Heat content of the products is greater than those of the reactant Heat content of the reactants is greater than those of the products None 12. The enthalpies of all elements in their standard states are: Unity Zero Always positive Always negative None 13. Which of the following is not a state function? Pressure Volume Temperature Heat None 14. Born-Haber's cycle is used to determine the: Combustion energy Decomposition energy Lattice energy Formation energy None 15. The number of fundamental ways for transferring energy into or out of system is: 1 2 3 4 None 16. Work is product of force and: Volume Time Displacement Pressure None 17. The spontaneous reaction are usually: Exothermic Fast Endothermic Both (a) and (b) None 18. At constant Volume, heat of reaction is represented by: Delta H Delta E Delta S Delta G None 19. The smallest unit of heat energy is: Calorie Joule Erg Kilo Joule None 20. At constant pressure, heat of reaction is represented by: Delta H Delta E Delta S Delta P None 21. In thermochemistry force displacement work is replaced by: Pressure volume work Pressure temperature work Temperature volume work None of these None 22. The net change in energy in a chemical reaction is same whether it takes place directly or indirectly. It is called: Henry's law Charlie's law Hess's law Graham's law None 1 out of 5 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-8 Chemical Equilibrium Welcome To Your Quiz "Ch-8 Chemical Equilibrium" Click on "Start Quiz" To Continue... 1. The value of pH and pOH of pure water at 25°C is approximately: 14 7 1 x 10-14 1 x 10 14 None 2. Conjugate acid of a very strong base is relatively: Very strong acid Weak acid Very weak acid strong acid None 3. Molarity of pure water is: 1 18 55.5 6 None 4. By adding NH4CI to NH4OH solution, the ionization of NH4OH: Increases Decreases Remain same Increases 100 times None 5. When Kc value is small, the equilibrium position is: Towards left Towards right Remains unchanged None of these None 6. A basic buffer solution can be prepared by mixing: A strong acid and salt with weak base Weak base and its salt with strong acid Strong base and its salt with weak acid Weak acid and its salt with strong base None 7. The term pH was introduced by: Henderson Sorenson Goldstein Thomson None 8. The solubility of KCIO3 in water is suppressed by adding: NaCIO3 NaCl KMNO4 KCI None 9. The ionic product of water will increase if: H+ ions are added OH ion are added Temperature is increased H+ and OH ions are added in equal amount. None 10. Which of the following factor affects on equilibrium constant? Change in temperature Change in concentration Change in Pressure Change in volume None 11. Which one of the following salt dissolves in water to form a solution with pH greater than 7? NaCl CuSO4 Na2CO3 NH4CI None 12. pH of milk is 6.5, its pOH will be: 14 7.5 7 None of these None 13. Formation of NH3 is an exothermic reaction. Low temperature favors forward reaction. However, in Haber's process temperature used is: 200°C 300°C 400°C 500°C None 14. When KCI is added to a saturated solution of KCIO3, the equilibrium is shifted to the: Forward direction Backward direction Not affected All of these None 15. pH of rain water is: 5,5 6.0 6.2 6.4 None 16. Strength of an acid can be determined by: pKa pH Ka All of these None 17. Solubility of Ca(OH)2 is exothermic, its solubility will increase: At high temperature At low temperature Temperature independent None None 18. Buffer action can be explained by: Common ion effect Law of mass action Le-Chatlier's principle All of these None 19. pH of a buffer solution having 0.01M CH3COONa and 0.1M CH3COOH (pKa = 4.74) is: 4.74 3.74 5.74 0 None 20. The pH of soft drink is: >7 <7 7 0 None 21. The pH of human blood is: 7.0 7.35 7.85 6.65 None 22. Almost forward reaction is complete when: Kc is very large Kc is very small Moderate Kc value None of these None 23. Equilibrium constant for gaseous equilibrium is represented by: Ka Kc Kx Kp None 24. The suppression or ionization of weak acid or a weak base by adding one of its own ions is: Buffer action Common ion effect Buffer capacity Ionization effect None 25. Law of mass action was derived by Guldberg and wage in: 1909 1906 1846 1864 None 1 out of 5 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-9 Solutions Welcome To Your Quiz "Ch-9 Solutions" Click on "Start Quiz" To Continue... 1. Depression in the freezing point is directly proportional to: Molarity of solution Molality of solution Molality of solvent None None 2. Benzene - ether can form: Ideal solution Non- ideal solution Buffer solution None of these None 3. In a mixture of 28 grams of N2 and 96 grams of O2 the mole fraction of N2: 1.1 0.51 0.25 0.11 None 4. The number of moles of solute per kilogram of solvent is called: Molality Molarity Mole-fraction Normality None 5. 0.1 molar of solute dissolved in 100g of the solvent will be: 0.1 molar 1.0 molal 0.5 molal none of these None 6. The amount of NaOH required to prepared 250 cm³ of 1M solution in grams is: 10 15 20 25 None 7. The azeotropic mixture of solution showing positive deviation can be distilled at _____ boiling point. Maximum Minimum No sharp None of these None 8. The hydration energy of Br- ion is _______ than F- ion: Equal to Smaller than Greater than None of these None 9. The molal boiling point elevation depends upon. Nature of solvent Vapour pressure of solution Nature of solute pH of solution None 10. An aqueous solution of potassium acetate (CH3OОK) is: Acidic Basic Neutral Amphoteric None 11. 2g of NaOH is dissolved in 500 cm³ of solution. The molarity of the solution is: 2.0 M 1.0 М 0.2 M 0.1 M None 12. In a mixture of 7g of N2 and 8g of O2 the mole fraction of O2 is: 1 0.2 0.5 0.7 None 13. Cheese and butter are the example of solution of: Liquid in liquid Solid in solid Liquid in solid Solid in liquid None 14. Water of crystallization of CuSO4 is: 2 5 6 10 None 15. The critical solution temperature of phenol-water system is: 35.6°C 49.5°C 57.8°C 65.9°C None 16. The mass of Glucose required to prepare 1 dm³ of 20% glucose solution is: 18g 180g 36g 200g None 17. Which one of the following is an ideal solution: C2H5OH and H2O C6H6 and CCl4 CHCl3 and (CH3)2 CO H2O and HCI None 18. 18 g glucose is dissolved in 90 g of water. The relative lowering of vapour pressure is equal to: 1/5 5.1 1/51 6 None 19. Which of the following concentration unit is used for very dilute solutions: Molarity Normality Molality ppm None 20. Which of the following is affected by temperature change: Molality Molarity Mole fraction None of these None 21. Hydrolysis of CH3COOK will produce: Acidic solution Basic solution Neutral Solution None of these None 22. The substance which has water of crystallization in it, is called: Hydrate Hydride Hydrolysis Complex None 23. The molarity of 2% W/V NaOH solution is: 2 0.25 0.05 0.5 None 24. Which one of the following salts do not hydrolyse: CuSO4 Na2CO3 Na2SO4 Al2(CO3)3 None 25. If 9.8g H2SO4 is present in one dm3 of solution, the solution is: 0.1 N 0.1 M 0.1 m 0.5 M None 26. An aqueous solution boils at 100.52°C. It should freeze at: 0°C -1.86°C -2°C +1.86°C None 27. Which has maximum freezing point: 1 m NaCl 1 m KCl 1 m CaCl2 1 m Urea None 28. Which cation has least heat of hydration: Li + Na + K + Mg +2 None 29. 10% aqueous solution of glucose freezes at: 0°C Less than 0°C Greater than 0°C Greater than 10°C None 30. A mixture of benzene and toluene form: Ideal solution Non - ideal solution Azeotropic mixture Suspension None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-10 Electrochemistry Welcome To Your Quiz "Ch-10 Electrochemistry" Click on "Start Quiz" To Continue... 1. The electrolyte KOH is used in cell: Lead accumulator Ni - Cd cell Alkaline battery Silver oxide battery None 2. In the reaction 2Fe + 3Cl2 ------> 2FeCIз: Fe is reduced Fe is oxidized Cl2 is oxidized None of these happens None 3. Oxidation state of hydrogen in CaH2 is: +1 -1 +2 0 None 4. Cu metal can be purified in electrolytic cell by making the impure Cu as: Anode Cathode Anode and Cathode Depends upon nature of solution None 5. Fuel cells convert chemical energy into: Heat energy Light energy Electrical energy Mechanical energy None 6. Nelson's cell and Down's cell are example of: Electrochemical cell Galvanic cell Electrolytic cell None of these None 7. The oxidation number of Cr in K2Cr2O7 is: +14 +12 +6 +13 None 8. The electrolyte used in fuel cell is: Aqueous NaCl Molten NaCI KOH NaNO3 None 9. Electrode potential of S.H.E arbitrarily taken in volts is: 0.00 1.00 0.01 0.50 None 10. Which one is not an electrolyte: Aqueous NaCl Aqueous CuSO4 Cu metal H2SO4 None 11. E.M.f of Zn-Cu cell is: 0.0V 0.5 V 1.0V 1.10V None 12. The highest reduction potential in the electrochemical series is of F2 and its value is: +3.87V -3.87V +2.87 V -2.87V None 13. Percentage of H2SO4 used in lead accumulator is: 40% 25% 30% 50% None 14. Cathode in NICAD cell is: Ag2O NiO2 Cd Zn None 15. The extraction of Na-metal by electrolysis of fused NaCl is carried out in: Down's cell Fuel cell Nelson's cell Voltaic cell None 16. Sulphur has the highest state in: SO2 SO3 H2S H2SO3 None 17. In rusting of iron shown by the reaction 4Fe + 302→2Fe2O3, Iron is: Precipitated Reduced Hydrolyzed Oxidized None 18. When aqueous NaCl is electrolyzed, which of the following get discharged at cathode: H+ Na+ OH Cl- None 19. A decrease in oxidation number is called: Oxidation Reduction Neutralization e.m.f None 20. Oxidation state of carbon in glucose (C6H1206) is: 0 1 2 4 None 21. Galvanic cells which cannot be re-charged are called: Diffused cells Secondary cells Tertiary cells Primary cells None 22. Consider the following reaction: Zn + Cu2+ → Zn2+ + Cu With reference to the above, which one of the following is the correct statement? Zn is reduced to Zn 2+ ions Zn is oxidised to Zn 2+ ions. Zn 2+ ions are oxidised to Zn. Cu 2+ ions are oxidized to Cu. None 23. Reduction never involves: gain of electrons decrease in oxidation number loss of electrons decrease in valency of electropositive component None 24. Which of the following has same oxidation state in all its compounds: Be Br Cl N None 25. The overall positive reaction potential value predicts that process is: Not feasible Feasible Impossible No identification None 26. In which of the following compounds oxidation number of sulphur is negative: SO2 H2SO4 H2S Na2SO4 None 27. Which of the following is a primary cell: Fuel cell Lead Accumulator Alkaline dry ceall Daniel cell None 28. Which of the following is a reducing agent in following reaction: P + HNO3 -----> H3PO4 + NO + H2O Phosphorus Nitrogen Nitric acid water None 29. When brine solution is electrolysed which of the following ions get discharged at anode: OH- Cl- Na+ H+ None 30. The change in the oxidation state of nitrogen in the following reaction is: Cu + HNO3 -----> Cu(NO3)2 + NO2 + H2O +5 to -2 +5 to +4 +5 to 0 0 to -4 None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-11 Reaction kinetics Welcome To Your Quiz "Ch-11 Reaction kinetics" Click on "Start Quiz" To Continue... 1. In zero order reaction, the rate is independent of: Temperature of reaction Concentration of reactants Concentration of product None of these None 2. The order of reaction of O3 + NO ----> NO2 + O2 is: 1 2 3 0 None 3. Decomposition of nitrogen pentaoxide has order of reaction: Zero First Second Third None 4. The catalyst used for the reaction HCOOH -----> H2+CO2 is: Copper Alumina Silica Iron None 5. Sugar solution hydrolyses to glucose and fructose in the presence of enzyme: Urease Invertase Zymase None None 6. If 75% of any given amount of radioactive element disintegrates in 60 minutes the half life radioactive element is: 20 minutes 30 minutes 40 minutes 25 minutes None 7. With increase of 10°C temperature, the rate of reaction becomes double. This increase in rate of reaction is due to: Decrease in the activation energy of reaction Decrease in number of collision between the molecules Increase in activation energy of reactants Increase in number of effective collision None 8. If the rate equation of reaction 2 A + B → Product Rate = k [A]² [B] and A is present in large excess, then order of reaction is: 1 2 3 None None 9. The energy of activated complex is: Greater than the reactants and products Less than the reactants and products Equal to the products Equal to the reactants None 10. Indicate the enzyme which catalyses the following: C6H1206 ----> 2C2H5OH+2CО2 Diastase Zymase Urease Invertase None 11. Which of following is an example of homogenous catalysis? Formation of ghee from oil Formation of SO3 in contact process Hydrolysis of ester Formation of NH3 in Haber process None 12. Hydrolysis of Tertiary butyl bromide has order of reaction: First order Pseudo first order Second order Third order None 13. If the rate of decay of radioactive isotope decreases from 200 cpm to 25 cpm after 24 hours.What is its half life: 3 hours 4 hours 6 hours 8 hours None 14. The rate of reaction between two specific time intervals is called: Rate of reaction Average rate Instantaneous rate None None 15. The half life of zero order reaction is: Proportional to initial concentration of reactants Independent of initial concentration of reactant Inversely proportional to initial concentration of reactant None of these None 16. Photo chemical reactions are: Zero order First order Second order Third order None 17. The energy of activation for a reaction by using catalyst is: Increased Decreased Not changed Moderate None 18. Which type of metals are usually used as catalyst: Coinage metal Alkali metals Transition metals Alkaline earth metals None 19. Which technique is used to determine the absorption of radiations: Spectrometry Dilatometric method Refractrometric method Optical rotation method None 20. Which property of a liquid is measured by polarimeter: Conductance Refractive index Optical activity Change in volume None 21. In specified conditions the rate of consumption of N2O5 in the reaction 2N2O5 ----> 4NO2 + O2 is 0.5 mol N2O5 L-1.S-1. The rate of formation of NO2 is 0.5 4 2 1 None 22. A substance which increases the efficiency of a catalyst is termed as: Promoter Activator Retarder Super catalyst None 23. The number of atoms or molecules whose concentration determines the rate of a chemical reaction is called the molecularity of the reaction order of the reaction specific activity of the reaction rate constant of the reaction None 24. The rate of chemical reaction depends upon the nature of reactants because? Some of the reactants have high boiling point Some of the reactants are colored Energy of activation differs from one reaction to another Some of the reactants are solid at room temperature None 25. The rate of chemical reaction is independent of: Molecularity Temperature Nature of reactants Concentration of reaction None 26. Larger the surface area of the reactant molecules: Lower will be the rate of reaction Higher will be the rate of reaction The rate of reaction remains unaffected The rate may increase or decrease None 27. The minimum amount of energy required for an effective collision is called: Activation energy Internal energy Translational energy None None 28. None 29. None 1 out of 6 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-12 Periodic Classification of Elements & Periodicity Welcome To Your Quiz "Ch-12 Periodic Classification of Elements & Periodicity" Click on "Start Quiz" To Continue... 1. The number of electrons in valence shell of an element reflects its: Period Number Group Number Both None None 2. Generally metals form oxides: Acidic Basic Amphoteric None None 3. Variable valency is shown by: Group 1A Group 2A Group 7A group 1B None 4. keeping in view the sizes of atoms, which order is the correct one: Mg > Sr Ba > Mg Be > Mg Ra > Ba None 5. which one of the following oxides is amphoteric in nature: MgO Na2O SO2 ZnO None 6. Atomic number was discovered by Mosley in: 1913 1914 1915 1916 None 7. Non-metals usually exist as: liquids Gases Liquids or gases Waxy solids None 8. Ga has oxidation state: +3 +2 +4 +1 None 9. Hydrides can be classified into: Two types Three types Four types Five types None 10. Which of the following pairs are chemically dissimilar: Na and K Ba and Sr Zr and Hf Ca and Zn None 11. Which of the following has greatest metallic character: Mg Ca Al Cs None 12. Highest hydration energy is shown by: Na+ Mg+2 Al+3 Ga+3 None 13. Which of the following pair of atomic numbers represents 2A element: 3,11 3,12 4,20 3,20 None 14. Among the following elements the highest value of electron affinity is shown by: F Cl Br I None 15. Alkali metals in each period have: Smallest size Lowest Ionization Energy Highest Ionization Energy Lowest atomic radius None 16. Polymeric (Intermediate) hydride shall be formed by: Na K Be C None 17. The highest acidity is shown by: Mn2O7 Mn2O3 MnO2 MnO None 18. The covalent hydrides are usually: Liquids Gases Volatile Liquids or gases Waxy solids None 19. Which of the following oxides is Amphoteric in character: CaO CO2 SiO2 Sb2O3 None 20. Hydrogen can be placed with the element of group (IV-A) because both: Act as strong oxidizing agent Act as strong reducing agent Possess the property of catenation Form neutral oxides None 1 out of 4 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-13 s-Block Elements Welcome To Your Quiz "Ch-13 s-Block Elements" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-14 Group IIIA & Group IVA Elements Welcome To Your Quiz "Ch-14 Group IIIA & Group IVA Elements" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-15 The Halogens & Noble Gases Welcome To Your Quiz "Ch-15 The Halogens & Noble Gases" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-16 Fundamental Principals of Organic Chemistry Welcome To Your Quiz "Ch-16 Fundamental Principals of Organic Chemistry" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-17 Aliphatic Hydrocarbons Welcome To Your Quiz "Ch-17 Aliphatic Hydrocarbons" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-18 Aromatic Hydrocarbons Welcome To Your Quiz "Ch-18 Aromatic Hydrocarbons" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-19 Alkyl Halides Welcome To Your Quiz "Ch-19 Alkyl Halides" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-20 Alcohols, Phenols & Ethers Welcome To Your Quiz "Ch-20 Alcohols, Phenols & Ethers" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-21 Aldehyde & Ketones Welcome To Your Quiz "Ch-21 Aldehyde & Ketones" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-22 Carboxylic Acid Welcome To Your Quiz "Ch-22 Carboxylic Acid" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... Name Email Time's up Ch-23 Macro Molecules Welcome To Your Quiz "Ch-23 Macro Molecules" Click on "Start Quiz" To Continue... 1 out of 0 Thanks For Taking This Quiz - Please See Your Answers/Results Below After Entering Your Name & Email... 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