Question

The decomposition of PCl5(g) to PCl3(g) and Cl2(g) is endothermic, ΔrHo = 92.5 kJ mol^(-1), and nonspontaneous, ΔrGo = 37.18 kJ mol^(-1) at 25.0°C. a) At what temperature(s) will the decomposition become spontaneous? b) Determine the concentration equilibrium constant, Kc, of the reaction.

Name: the decomposition of pcl5g to pcl3g and cl2g is endothermic rho 925 kj mol1 and nonspontaneous rgo 3718 kj mol1 at 250oc a at what temperatures will the decomposition become spontaneous b de 71677
Uploaded: 2022-07-15T22:56:22-08:00
Duration: 3 min 31 s
Channel: David Collins
Description: the decomposition of pcl5g to pcl3g and cl2g is endothermic rho 925 kj mol1 and nonspontaneous rgo 3718 kj mol1 at 250oc a at what temperatures will the decomposition become spontaneous b de 71677

          The decomposition of PCl5(g) to PCl3(g) and Cl2(g) is endothermic, ΔrHo = 92.5 kJ mol^(-1), and nonspontaneous, ΔrGo = 37.18 kJ mol^(-1) at 25.0°C.

a) At what temperature(s) will the decomposition become spontaneous?
b) Determine the concentration equilibrium constant, Kc, of the reaction.

Added by Jeremiah S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

07/15/2022

Step 1

Given: - ΔrHo = 92.5 kJ mol^(-1) - ΔrGo = 37.18 kJ mol^(-1) at 25.0°C (298 K) - ΔrSo = 0.186 kJ mol^(-1) K^(-1) We know that ΔrGo = ΔrHo - TΔrSo Setting ΔrGo to 0 to find the temperature at which the reaction becomes spontaneous: 0 = 92.5 - T * 0.186 T = 92.5 / Show more…

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The decomposition of PCl5(g) to PCl3(g) and Cl2(g) is endothermic, ΔrHo = 92.5 kJ mol^(-1), and nonspontaneous, ΔrGo = 37.18 kJ mol^(-1) at 25.0°C. a) At what temperature(s) will the decomposition become spontaneous? b) Determine the concentration equilibrium constant, Kc, of the reaction.