Answer:
a. Not change the free energy value
b. Increase the free energy value
c. Decrease the free energy value
d. Decrease the free energy value
Explanation:
a. Adding a catalyst:
A catalyst is a substance that will reduce the activation energy of a reaction, it means that the reaction will occur fast. The values of enthalpy, entropy, and free energy are not affected by a catalyst, so ΔG remains the same.
b. Increasing [C] and [D]:
For a reversible reaction, the value of free energy can be calculated by:
ΔG = ΔG° + RT*lnK
Where ΔG° is the standard value for free energy, R is the gas constant, T is the temperature, and K is the constant of equilibrium, which in this case:
K = ([C]*[D])/([A]*[B])
When [C] and [D] increase, the value of K increases, and lnK also increases, then, the value of ΔG increases.
c. Coupling with ATP hydrolysis:
The free energy can be calculated by:
ΔG = ΔH - TΔS
Where ΔH is the change in enthalpy, and ΔS the change in entropy. The ATP hydrolysis is an exothermic reaction, so ΔH <0. When it is coupled, it will reduce the total value of ΔH, and because of that, the value of ΔG will decrease.
d. Increasing [A] and [B]:
As explained above, the increasing at [A] and [B] will decrease the value of K, so the value of lnK will decrease, and ΔG value will also decrease.
