Chemistry

Chemistry

Problem

At 298 K the equilibrium constant for the reaction C2H4(g)+H2(g)⇌C2H6(g)\text{C}_2\text{H}_4(g)+\text{H}_2(g) \rightleftharpoons \text{C}_2\text{H}_6(g) is K=9.6K=9.6. When the temperature is raised to 350 K, the value of the equilibrium constant drops to K=4.1K=4.1. What is the sign of ΔH∘\Delta H^{\circ} for the forward reaction? a) ΔH∘>0\Delta H^{\circ}>0 (endothermic) b) Cannot be determined from the information given c) ΔH∘<0\Delta H^{\circ}<0 (exothermic) d) ΔH∘=0\Delta H^{\circ}=0

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