Hydrogen sulfide can be formed in the following reaction: H₂(g) + ½S₂(g) ⇄ H₂S(g) ΔH°_rxn = −92 kJ
The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.

Question

Hydrogen sulfide can be formed in the following reaction: H₂(g) + ½S₂(g) ⇄ H₂S(g) ΔH°_rxn = −92 kJ The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.

Quizplus · Accepted Answer

The Answer of Hydrogen sulfide can be formed in the following reaction: H₂(g) + ½S₂(g) ⇄ H₂S(g) ΔH°_rxn = −92 kJ The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.

Hydrogen Sulfide Can Be Formed in the Following Reaction: H2(g)

Hydrogen Sulfide Can Be Formed in the Following Reaction: H₂(g)