Consider the following endothermic reaction 2H₂S(g) → 2H2(g) + S2 (g) where Kp = 1.67 x 10-7 What would happen to the eq

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Consider The Following Endothermic Reaction 2h S G 2h2 G S2 G Where Kp 1 67 X 10 7 What Would Happen To The Eq 1 (36.48 KiB) Viewed 21 times

Consider the following endothermic reaction 2H₂S(g) → 2H2(g) + S2 (g) where Kp = 1.67 x 10-7 What would happen to the equilibrium if we added some H₂(g)? Nothing will change No answer text provided. The equilibrium will shift left toward reactants: The equilibrium shifts right toward products Question 13 Consider the following endothermic reaction 2H₂S(g) + 2H2(g) + S2 (9) where K, = 1.67 x 10-7 What would happen to the equilibrium if we heated the reaction? The equilibrium will shift left toward reactants The equilibrium shifts right toward products No answer text provided. Nothing will change