Hydrogen sulfide can be formed in the following reaction: H₂(g) + S₂(g) H₂S(g) ; ΔH°_rxn = -92 kJ/mol
The equilibrium constant,K_P,is 106 at 1023 K. Estimate the value of K_P at 1218 K. (R = 8.314 J/K • mol)

Question

Hydrogen sulfide can be formed in the following reaction: H₂(g) +

Hydrogen sulfide can be formed in the following reaction: H<sub>2</sub>(g) + S<sub>2</sub>(g) H<sub>2</sub>S(g) ; ΔH°<sub>rxn</sub> = -92 kJ/mol The equilibrium constant,K<sub>P</sub>,is 106 at 1023 K. Estimate the value of K<sub>P</sub> at 1218 K. (R = 8.314 J/K • mol) A) 5.05 B) 18.8 C) 34.7 D) 88.9 E) 598

S₂(g)

H₂S(g) ; ΔH°_rxn = -92 kJ/mol
The equilibrium constant,K_P,is 106 at 1023 K. Estimate the value of K_P at 1218 K. (R = 8.314 J/K • mol)

Quizplus · Accepted Answer

The Answer of Hydrogen sulfide can be formed in the following reaction: H₂(g) + S₂(g) H₂S(g); ΔH°_rxn = -92 kJ/mol The equilibrium constant,K_P,is 106 at 1023 K. Estimate the value of K_P at 1218 K. (R = 8.314 J/K • mol)

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

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