For a reaction with ( H^ = -40.0

CHEMISTRY · Single correct · A Level · Chemistry · Chemical equilibria (Le Chatelier’s principle and Kc) · Chemical equilibria (Le Chatelier’s principle and Kc)

Problem

For a reaction with ΔH∘=−40.0 kJ mol−1\Delta H^\circ = -40.0\,\text{kJ mol}^{-1} and ΔS∘=−50 J mol−1 K−1\Delta S^\circ = -50\,\text{J mol}^{-1}\,\text{K}^{-1}, what is the approximate value of the ratio K700K350\frac{K_{700}}{K_{350}}, where the subscripts denote temperature in kelvins? (R=8.314 J mol−1 K−1R = 8.314\,\text{J mol}^{-1}\,\text{K}^{-1}) (a) 1×1031 \times 10^{3} (b) 11 (c) 1×10−31 \times 10^{-3} (d) 4×10−44 \times 10^{-4}

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