Grand Mock Test Chemistry 1st Year (AFNS) Leave a Comment / By abdulslambsn@gmail.com / July 21, 2025 Grand Mock Test Chemistry 1st Year (AFNS) Your Good Name: Your City: Email: 1. One mole of any gas at STP occupies the same volume because: All gases are ideal Pressure is constant Number of particles is constant Temperature is absolute None 2. The empirical formula of a compound is CHā. Its molar mass is 56 g/mol. What is its molecular formula? CāHā CāHā CāHā Cā Hāā None 3. If 10 g of calcium reacts with excess water, the volume of hydrogen produced at STP is: 5.6 dmĀ³ 11.2 dmĀ³ 22.4 dmĀ³ 1.12 dmĀ³ None 4. Which of the following has maximum number of atoms? 1 mole of Oā 1 mole of CHā 1 mole of HāO 1 mole of COā None 5. Which statement is incorrect regarding limiting reactant? It controls the amount of product It is always in lesser amount It is completely consumed It determines the theoretical yield None 6. In hydrogen spectrum, the Balmer series lies in: Infrared Ultraviolet Visible Microwave None 7. Which electron transition emits maximum energy? n=4 ā n=3 n=3 ā n=2 n=2 ā n=1 n=5 ā n=4 None 8. If the radius of 1st Bohr orbit is r, then radius of 3rd orbit is: 3r 6r 9r r/3 None 9. Energy of an electron in nth orbit is directly proportional to: 1/n nĀ² 1/nĀ² n None 10. The Uncertainty principle implies: Electron moves in a fixed path Momentum of electron is constant Exact position and momentum canāt be known simultaneously Energy levels are continuous None 11. Which of the following has the smallest atomic radius? Li B C O None 12. Ionization energy increases across the period because: Nuclear charge increases Atomic size increases Shielding effect increases Electronegativity decreases None 13. Which element has the highest electronegativity? O N Cl F None 14. Which ion has the largest size? Naāŗ MgĀ²āŗ Fā» OĀ²ā» None 15. The anomaly in IE trend from Be to B is due to: Half-filled orbital stability Full-filled orbital s to p sublevel transition Nuclear shielding None 16. The bond angle in NHā is less than that in CHā due to: Larger size of N Lone pair repulsion Smaller hybrid orbitals Greater electronegativity None 17. Which has a coordinate covalent bond? HCl NHāāŗ CHā HāO None 18. Hybridization of carbon in ethyne is: spĀ³ spĀ² sp None None 19. Which compound has the highest ionic character? NaCl MgClā AlClā BeClā None 20. Which gas deviates least from ideal behavior? COā NHā Hā SOā None 21. Compressibility factor (Z) for real gas is: Always 1 >1 at high pressure <1 at low pressure Always <1 None 22. Van der Waals constants 'a' and 'b' correct for: Temperature and volume Volume and pressure Intermolecular forces and volume Number of moles and temperature None 23. Which process shows increase in entropy? Freezing Condensation Evaporation Deposition None 24. According to kinetic theory, pressure is due to: Attraction among molecules Molecular collisions with walls Weight of molecules Speed of molecules None 25. Enthalpy is defined as: H = E - PV H = E + PV H = E Ć PV H = E / PV None 26. āH for endothermic reactions is: Negative Zero Positive Unpredictable None 27. Heat of formation of elements in standard state is: 1 0 Variable Negative None 28. In exothermic reactions: Bonds are broken āH is negative Heat is absorbed Potential energy increases None 29. Which has the highest bond energy? ClāCl HāH O=O CāC None 30. A reaction reaches equilibrium when: Reactants are fully consumed Forward rate = backward rate Products dominate Catalyst is added None 31. Increase in pressure favors: Side with more moles No effect Side with fewer moles Endothermic side None 32. In Haber process, high temperature decreases yield because: Activation energy increases Equilibrium shifts left Catalyst is deactivated Pressure decreases None 33. Which affects equilibrium constant? Temperature Pressure Volume Catalyst None 34. The equilibrium constant Kc is expression of: Rate Pressure Concentration Time None 35. Which acid is triprotic? HCl HNOā HāSOā HāPOā None 36. A buffer solution resists change in: Volume Pressure pH Temperature None 37. Which of the following is an acidic salt? NaCl KāSOā NaHSOā CHāCOONa None 38. Which is a Lewis acid? BFā NHā HāO OHā» None 39. Conjugate base of HCOāā» is: HāCOā COā COāĀ²ā» Hāŗ None 40. Electrolysis of molten NaCl gives: Na at cathode, Clā at anode Hā at cathode, Clā at anode Na at anode, Clā at cathode NaCl at both electrodes None 41. Oxidation occurs at: Cathode Anode Electrolyte Salt bridge None 42. Which is reduced in electrochemical cell? Anode Electrolyte Cathode Salt Bridge None 43. Which is reduced in electrochemical cell? Anode Electrolyte Cathode Salt Bridge None 44. Standard electrode potential of hydrogen electrode is: 1.00 V 0.00 V -1.00 V 0.50 V None 45. Which ion is discharged first at cathode? Naāŗ Kāŗ Hāŗ CaĀ²āŗ None 46. The unit of rate constant for first-order reaction is: molā»Ā¹ dmĀ³ sā»Ā¹ sā»Ā¹ mol dmā»Ā³ sā»Ā¹ mol sā»Ā¹ None 47. The rate of reaction depends upon: Thermodynamics Activation energy Product stability Electronegativity None 48. Catalyst increases the rate by: Increasing temperature Increasing concentration Lowering activation energy Increasing pressure None 49. For zero-order reaction, rate is: Dependent on concentration Independent of concentration Proportional to volume Decreases with time None 50. Rate constant doubles when temperature increases by 10Ā°C. This is explained by: Arrhenius equation Hessās law Le Chatelierās principle Boyleās law None 51. The half-life of a first-order reaction is: Directly proportional to concentration Inversely proportional to concentration Independent of concentration Depends on temperature None 52. A reaction is said to be elementary if: It occurs in multiple steps Activation energy is zero It occurs in a single step Rate is zero None 53. The collision theory fails to explain: Molecular orientation Activation energy Reaction order Rate constant None 54. A photochemical reaction is initiated by: Catalyst Heat Pressure Light None 55. In a reaction mechanism, the slowest step is: Fast step Rate-determining step Catalytic step Final step None 56. Order of a reaction is determined by: Balanced equation Catalyst used Experimental data Number of reactants None 57. For a second-order reaction, units of rate constant are: mol-Ā¹ dm3 s-Ā¹ s-Ā¹ mol dm-3 s-Ā¹ dm3 mol-Ā¹ s-Ā¹ None 58. s-Ā¹In reversible reactions, chemical equilibrium is: Static Dynamic Only forward Only backward None 59. When activation energy is low, the reaction is: slow Endothermic Fast Non-spontaneous None 60. A positive catalyst: Increases yield Increases rate Changes DeltaH Increases activation energy None 1 out of 6 Thanks For Submitting Your Quiz !!
