Question

For the reaction A+B↽−−⇀C+DA+B↽−−⇀C+D , assume that the standard change in free energy has a positive value. Changing the conditions of the reaction can alter the value of the change in free energy (Δ????)(ΔG) . Classify the conditions as to whether each would decrease the value of Δ????ΔG , increase the value of Δ????ΔG , or not change the value of Δ????ΔG for the reaction. For each change, assume that the other variables are kept constant.

Answer 1

Explanation:

Gibbs free energy (G) is dependent upon the enthalpy (H) , temperature (T) and entropy (S) as shown in the equation below;

ΔG =  ΔH   −  TΔS

The factors affect ΔG of a reaction are given below;

Decrease the Value of G

- Positive ΔH and Positive ΔS at high temperatures.

- Negative ΔH and Negative ΔS at low temperatures.

Would not change the value of G

- Negative values of ΔH and Positive values of ΔS; (at all temperatures,  ΔG would be Negative)

- Positive values of ΔH and Negative values of ΔS; (at all temperatures,  ΔG would be positive)

Increase the Value of G

- Positive values of ΔH and Positive ΔS at low temperatures.

- Negative ΔH and Negative ΔS at high temperatures.

Answer 2

What are the answer choices