Consider the following reaction:
2 NO(g) + Cl2(g) → 2 NOCl(g)
The enthalpy change at 298 K for this reaction is ΔH°rxn = -75.54 kJ/mol.
Under the same conditions, the entropy change for the reaction is ΔS°rxn = -116.6 J/mol-K.
Calculate the value of Keq for this reaction at 671 K. Assume that ΔH°rxn and ΔS°rxn are the same at 671 K as they are at 298 K. Use R = 8.314 J/(mol·K) for the value of the gas constant.
a) At this temperature, Keq = 1.62e+00.
b) At this temperature, Keq = 1.41e+07.
c) At this temperature, Keq = 1.00e+00.
d) At this temperature, Keq = 1.50e+03.
e) At this temperature, Keq = 6.16e-01.