1. Which of the following relations is correct?[IOM 2007]
- ΔG° = RT lnK
- ΔG° = -RT lnK
- ΔG° = -RT logK
- ΔG° = RT logK
(b) The correct thermodynamic relation is ΔG° = -RT lnK, where K is the equilibrium constant. 2. Gibbs free energy (G), enthalpy (H) and entropy (S) are related by[IOM 2005, MOE 2009]
- G = H + TS
- G = H - TS
- G - S = TH
- S = H - GT
(b) The fundamental relation is G = H - TS, defining Gibbs free energy. 3. Decrease in the free energy of a reacting system indicates the reaction to be
- A reversible reaction
- An endothermic reaction
- A spontaneous reaction
- A primary reaction
(c) A negative ΔG (decrease in free energy) indicates spontaneity. 4. According to the first law of thermodynamics[MOE 09]
- Heat cannot flow from colder to hotter body
- Energy can neither be created nor destroyed
- The efficiency of a heat engine can never be 100%
- Entropy of universe is increasing
(b) First law states the conservation of energy principle. 5. According to ΔG = ΔH - TΔS, spontaneity occurs when ΔG is[IOM 2008, BPKIHS]
- Positive
- Negative
- Zero
- Infinite
(b) Negative ΔG indicates spontaneous reactions. 6. The sum of internal energy and pressure-volume energy is[BPKIHS 2006]
- First law of thermodynamics
- Enthalpy
- Entropy
- None
(b) Enthalpy (H) = Internal energy (E) + PV. 7. In endothermic reactions, the reactants
- Have less energy than products
- Have more energy than products
- Have same energy as products
- Are at lower temperature than products
(a) Endothermic reactions absorb heat, making products higher in energy. 8. For the reaction Fe₂O₃ + 3CO → 2Fe + 3CO₂, which relation is correct?[BPKIHS]
- ΔH = ΔE
- ΔH = ΔE - RT
- ΔH = ΔE + RT
- ΔH = ΔE + 2RT
(d) ΔH = ΔE + ΔnRT, where Δn = +2 (gas moles increase by 2). 9. PV = nRT is applicable to[MOE 2062]
- Isothermal changes
- Adiabatic changes
- Both (a) and (b)
- None
(a) Ideal gas law strictly applies to isothermal (constant T) conditions. 10. When liquid boils, there is increase in[BPKIHS]
- Entropy
- Heat of vaporization
- Kinetic energy
- Potential energy
(a) Boiling increases molecular disorder ⇒ entropy (ΔS) increases. 11. Which can be converted to useful work?[BPKIHS 2002]
(c) Gibbs free energy (ΔG) represents maximum reversible work. 12. For the process: Dry ice → CO₂(g)[Bangladesh 2008]
- ΔH = +ve, ΔS = -ve
- Both ΔH, ΔS = -ve
- Both ΔH, ΔS = +ve
- ΔS = +ve, ΔH = -ve
(c) Sublimation is endothermic (ΔH>0) and increases disorder (ΔS>0). 13. H, E, P and V are related as
- H = E + P - V
- H = E + PV
- H = E - PV
- H = P - EV
(b) Enthalpy (H) = Internal energy (E) + Pressure-Volume work (PV).