Gibbs Free Energy Problems

For all of the problems below, here is the reaction: A <=> B. Assume in each case that the temperature is 300 K.

1. If the Delta G^{0'} for this reaction is - 10 kJ/mol, and there is twice as much B as A, will the reaction go forward as written?

2. If the Delta G^{0'} for this reaction is + 10 kJ/mol, what is the ratio of B/A that will make the reaction at equilibrim? How does one tip the reaction in the direction of backwards?

3. At equilibrium, there is 5 times as much B as A. What is the G^{0'} for this reaction?

4. If the Delta G^{0'} for this reaction is + 5 kJ/mol and the concentration of B is 0.3M, what is the minimum concentration of A required to make the reaction favorable?

5. If the Delta G^{0'} for this reaction is + 5 kJ/mol, what is the ratio of B to A at equilibrium?

6. If the Delta G for the reaction is 8 kJ/mol when there is 0.5M A and 0.2M B, what is the equilibrium concentration of A and B?

For all of the problems below, here is the reaction: A <=> B. Assume in each case that the temperature is 300 K, except as noted.

1. What is the Delta G^{0'} for a reaction if the Delta G is -20 kJ/mol when there is 5 times as much A as B?

2. When the Delta G for a reaction is -10 kJ/mol and the Delta G^{0'} is -10 kJ/mol, what is the ratio of A to B?

3. If the ratio of A/B in #1 stays the same, what happens to the Delta G when the temperature drops 50 degrees?

4. A reaction is favorable when there is twice as much A as B and also when there is twice as much B as A. Is this possible? If not, why not. If so, explain.