Question

A)

A reaction has an equilibrium constant of Kp=0.280 at 44 ∘C.

Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 3.35 kJ -3.35 kJ 0.404 kJ 0.466 kJ

B)

Above what temperature does the following reaction become nonspontaneous?

FeO(s) + CO(g) → CO₂(g) + Fe(s) ΔH= -11.0 kJ; ΔS = -17.4 J/K

Above what temperature does the following reaction become nonspontaneous?

FeO(s) + CO(g) → CO₂(g) + Fe(s) = -11.0 kJ; = -17.4 J/K

191 K

298 K

632 K

This reaction is nonspontaneous at all temperatures.

This reaction is spontaneous at all temperatures.

C)

Estimate ΔG°_rxn for the following reaction at 387 K.

HCN(g) + 2 H₂(g) → CH₃NH₂(g) ΔH°= -158.0 kJ; ΔS°= -219.9 J/K

Estimate ΔG°_rxn for the following reaction at 387 K.

HCN(g) + 2 H₂(g) → CH₃NH₂(g) ΔH°= -158.0 kJ; ΔS°= -219.9 J/K

+72.9 kJ

+61.9 kJ

-243 kJ

-72.9 kJ

+243 kJ

Answer 1