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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 kThe 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»

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.


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