Two different reactions were studied at equilibrium under separate…

CHEMISTRY · Subjective · A Level · Chemistry · Thermodynamics · Thermodynamics

Problem

Two different reactions were studied at equilibrium under separate constant-temperature conditions, giving the linear relationships shown below: Reaction X: ΔG∘ (J mol−1)=−1.50×103 ln⁡K+50\Delta G^\circ\,(\text{J mol}^{-1}) = -1.50 \times 10^3\,\ln K + 50 Reaction Y: ΔG∘ (J mol−1)=−3.00×103 ln⁡K−120\Delta G^\circ\,(\text{J mol}^{-1}) = -3.00 \times 10^3\,\ln K - 120 Which reaction was studied at the higher temperature? Support your answer with a numerical comparison.

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