BAED-CHEM2122 General Chemistry 2
Q1. Specific heat of substance A (25 J for 5.0 g, ΔT = 2.0°C):
Answer: 2.5 J/g°C
Q2. Phase with greatest motion and least order:
Answer: Gas
Q3. ΔH positive (endothermic processes):
Answer: 3 (Water boils) and 4 (Dry ice sublimes)
Q4. Reaction rate vs. spontaneity:
Answer: True
Q5. Free energy (ΔG) for reaction (ΔH = -104 kJ, ΔS = -60.8 J/K, T = 30°C):
Answer: -85.6 kJ, spontaneous
Q6. Temperature measures average kinetic energy:
Answer: Kinetic
Q7. Equation relating enthalpy, temperature, entropy:
Answer: Gibbs Free Energy
Q8. ΔH in endothermic reactions:
Answer: True
Q9. Heat transfer direction (hot to cold):
Answer: Always
Q10. Energy to raise 1g water by 1°C:
Answer: Calorie
Q11. SI unit of energy:
Answer: Joule
Q12. Catalyst role:
Answer: Lowers activation energy
Q13. Entropy definition:
Answer: True
Q14. Second law of thermodynamics:
Answer: Entropy always increases
Q15. Effect of pressure increase on ( N₂ + 3H₂ ⇄ 2NH₃ ):
Answer: NH₃ increases
Q16. Equilibrium definition (forward = reverse rate):
Answer: Chemical Equilibrium
Q17. Adding SO₃ to ( 2SO₂ + O₂ ⇄ 2SO₃ ):
Answer: Shift equilibrium left
Q18. Removing O₂ from same reaction:
Answer: Shift equilibrium left
Q19. Equilibrium conditions:
Answer: Forward/reverse rates equal, concentrations constant
Q20. Reversible reaction symbol:
Answer: Reversible
Q21. Increasing SO₂ shifts equilibrium:
Answer: Right
Q22. Increasing pressure on ( 2NO + O₂ ⇄ 2NO₂ ):
Answer: Yield of NO₂ increases
Q23. False equilibrium statement:
Answer: Reactant concentration equals product concentration
Q24. Highest entropy:
Answer: Hot gas
Q25. Temperature increase on ( H₂ + Cl₂ ⇄ 2HCl ):
Answer: Shift left
Q26. Conjugate base in ( HCO₃⁻ + HCl → H₂CO₃ + Cl⁻ ):
Answer: Cl⁻
Q27. Conjugate acid in ( HSO₄⁻ + H₂O → H₃O⁺ + SO₄²⁻ ):
Answer: H₃O⁺
Q28. Conjugate base in ( CO₃²⁻ + H₂O → HCO₃⁻ + OH⁻ ):
Answer: OH⁻
Q29. Transfer between conjugate pairs:
Answer: Proton
Q30. Ion in basic solution:
Answer: OH⁻
Q31. Bronsted-Lowry acid definition:
Answer: Donates H⁺
Q32. Neutralization products:
Answer: H₂O + Ionic Salt
Q33. Strong acid + strong base result:
Answer: pH-neutral substance
Q34. Conjugate acid definition:
Answer: Base after accepting H⁺
Q35. Ksp units for ( Ag₂CO₃ ):
Answer: mol³ dm⁻⁹
Q36. Endothermic reaction solubility:
Answer: Solubility and Ksp increase
Q37. Molar solubility of ( PbI₂ ):
Answer: 1.40 × 10⁻⁸ mol³ dm⁻⁹
Q38. Solubility of ( Ag₂CrO₄ ):
Answer: 1.31 × 10⁻⁴ M
Q39. Ksp units for ( AgCl ):
Answer: mol² dm⁻⁶
Q40. Expression for ( Sn(OH)₂ ):
Answer: 4s³ = Ksp
Q41. Pressure effects on equilibrium:
Answer: Gaseous substances
Q42. Negative electrode in ( Zn/Zn²⁺ // Cu²⁺/Cu ):
Answer: Zinc
Q43. Electron flow direction:
Answer: Anode to cathode
Q44. Oxidation at anode ( Ag⁺/Ag = 0.80V, Ni²⁺/Ni = -0.25V ):
Answer: Ni → Ni²⁺ + 2e⁻
Q45. Iron in copper nitrate solution:
Answer: Iron becomes copper-plated
Q46. Supersaturated solution:
Answer: Dissolve more solute than equilibrium allows
Q47. Solubility definition:
Answer: Concentration of dissolved solute
Q48. Precipitation condition:
Answer: Qsp = Ksp
Q49. Temperature effect on exothermic reactions:
Answer: Solubility and Ksp decrease
Q50. Unsaturated solution definition:
Answer: Can dissolve more solute
