Question

If the value of ΔG0 is -2502 J/mol and K is 2, what is the temperature of the reaction that is occurring?

(a) 200 k

(b) 101 k

(c) 100 k

(d) 300 k

The question was posed to me in class test.

The origin of the question is Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G in portion Equilibrium of Chemistry – Class 11

Answer 1

The correct option is (c) 100 k

The best I can explain: We know that ΔG0 = – RT lnKc, where ΔG0 is the standard Gibbs free energy, R is universal gas constant, T is the temperature and KC is equilibrium constant; substituting ΔG0 as -2502 J/mol, we get -2502 J/mol = -8.314J mol^–1K^–1 × T ln2 = 2502 J/mol = T = 2502/2.502 = 100 k.