Assignment 3: Gibbs Free Energy
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 G0' 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 G0' 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 G0' for this
reaction?
4. If the Delta G0' 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 G0' 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 G0' 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 G0' 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.