Question

There is a similar question online but the choices aren't the same. Please help me with this questions:

For the reaction given below, assume that the standard change in free energy has a positive value.

A+B arrow sign right/under arrow sign left C+D

Changing the conditions of the reaction can alter the value of the change in free energy (ΔG). Sort the following conditions as to whether each would decrease the value of ΔG, increase the value of ΔG, or not change ΔG for the reaction. For each change, assume that the other variables are kept constant.

Category:

Decrease Delta G Increase Delta G No effect on Delta G

Choices:

Coupling with ATP hydrolysis

Increasing (C) and (D)

Increasing (A) and (B)

Adding a catalyst

Answer 1

∆G °=∆H°-T∆S is positive ,that mean ∆H should be positive ,so the reaction is endothermic means we need provide heat to make the reaction forward.

A + B --> C + D [∆G°= +ve, ∆H°= -ve]

If temprature increases, ∆G decrease reaction will go forward

If temprature decrease , ∆G increases Reaction will go backwards.

If ∆G become zero, than the reaction will come in equilibrium.