Answer :
In this question, we are asked to determine which value of TΔS would make this reaction be spontaneous, and to determine that, we have to use the Gibbs Free Energy formula, which is:
ΔG = ΔH - TΔS
Where:
ΔG is Gibbs free energy
ΔH is change in enthalpy, which our value is 2 kJ
TΔS is Temperature and change in Entropy
If the result of this formula gives a positive number, the reaction will be non-spontaneous
If the result of this formula gives a negative number, the reaction will be spontaenous
Therefore we need to choose a value in which the result of the formula will give a NEGATIVE value, let's try:
A. 3 kJ
ΔG = 2 - 3
ΔG = -1
B. 2 kJ
ΔG = 2 - 2
ΔG = 0
C. - 2 kJ
ΔG = 2 - (-2)
ΔG = 4
D. -3 kJ
ΔG = 2 - (-3)
ΔG = 5
Therefore the only option that presents a negative value as result is letter A
