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## Relationship between K, Q and G MCQs

**1. In a reaction, if the value of Gibbs free energy is greater than zero what does it infer?**

a) K is greater than 1

b) K is less than 1

c) K is equal to 1

d) Cannot deduce K from Gibbs free energy

**Answer: **K is less than 1

**2. When is a reaction nonspontaneous?**

a) Gibbs free energy is positive

b) Gibbs free energy is negative

c) Gibbs free energy is zero

d) Does not depend on Gibbs free energy

**Answer: **Gibbs free energy is positive

**3. What did the Q depicted in the equation; ΔG = ΔG0 + RT lnQ?**

a) reaction coefficient

b) reaction quotient

c) equilibrium constant

d) free energy

**Answer: **reaction quotient

**4. If the value of Gibbs free energy for a reaction is 20J/mol, the reaction is ___________**

a) spontaneous

b) nonspontaneous

c) may be spontaneous

d) may not be spontaneous

**Answer: **nonspontaneous

**5. ****For a reaction, K**_{c}** = 3.81 × 10**^{–3}** and ΔG**_{0}** = 13.8 kJ/mo****l. Then what is the value of R?**

_{c}

^{–3}

_{0}

a) -8.314J mol^{–1}K^{–1}

b) 8.314J mol^{–1}K^{–1}

c) cannot say as the temperature is not given

d) -8.314J mol^{–1}

**Answer: **8.314J mol^{–1}K^{–1}

**6. What happens when reaction quotient is equal to the equilibrium constant?**

a) the reaction proceeds in the forward direction

b) the reaction proceeds in the backward direction

c) the reaction reaches equilibrium

d) cannot predict

**Answer: **the reaction reaches equilibrium

**7. ****Is a relationship between reaction quotient and Gibbs ****free energy at a temperature T?**

a) ΔG = ΔG_{0} + RT lnQ

b) ΔG = ΔG_{0} + RT lnk

c) ΔG = ΔG_{0} + R lnQ

d) ΔD = ΔG_{0} + RT lnQ

**Answer: **ΔG = ΔG_{0} + RT lnQ

**8****. In a reaction, at 300k, K**_{C}** is given as 2 x 10**^{13}**, then what is the value of ΔG?**

_{C}

^{13}

a) – 7.64 × 10^{4} J

b) – 7.64 × 10^{4} J mol^{–1}

c) – 7.64 × 10 J mol^{–1}

d) – 7.64 × 10^{4} mol^{–1}

**Answer: **– 7.64 × 10^{4} J mol^{–1}

**9. ****For a chemical reaction, the value of ΔG**_{0}** is -831.4 J/mol. Then what is the value of K**_{C}** at 100 k?**

_{0}

_{C}

a) 1.0077

b) 1.077

c) 1.007

d) 2.7

**Answer: **2.7

**10. ****If the value of ΔG**_{0}** is -2502 J/mol and K is 2, what is the temperature of ****the reaction that is occurring?**

_{0}

a) 200 k

b) 101 k

c) 100 k

d) 300 k

**Answer: **100 k