Hydrogen sulfide can be formed in the following reaction: H 2 (g) + S 2 (g) H 2 S(g) $\Delta$H° rxn = -92 kJ The equilibrium constant K p = 106 at 1023 K. Estimate the value of K p at 1218 K.

The Answer of Hydrogen sulfide can be formed in the following reaction: H 2 (g) + S 2 (g) H 2 S(g) $\Delta$H° 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: H 2 (g) + S 2 (g) H 2 S(g) $\Delta$H° rxn = -92 kJ The equilibrium constant K p = 106 at 1023 K. Estimate the value of K p at 1218 K.

The Answer of Hydrogen sulfide can be formed in the following reaction: H 2 (g) + S 2 (g) H 2 S(g) $\Delta$H° rxn = -92 kJ The equilibrium constant K p = 106 at 1023 K. Estimate the value of K p at 1218 K.

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

Question 72

Multiple Choice

Hydrogen sulfide can be formed in the following reaction: H₂(g) + $Hydrogen sulfide can be formed in the following reaction: H2(g) + S2(g) H2S(g) \Delta H°rxn = -92 kJ The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K. A) 5.05 B) 18.8 C) 34.7 D) 88.9 E) 598$ S₂(g) $Hydrogen sulfide can be formed in the following reaction: H2(g) + S2(g) H2S(g) \Delta H°rxn = -92 kJ The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K. A) 5.05 B) 18.8 C) 34.7 D) 88.9 E) 598$ H₂S(g) $\Delta$ H°_rxn = -92 kJ
The equilibrium constant K_p = 106 at 1023 K. Estimate the value of K_p at 1218 K.