A biochemical reaction is studied at a constant

CHEMISTRY · Multi-part · A Level · Chemistry · Thermodynamics · Thermodynamics

Problem

A biochemical reaction is studied at a constant, unknown temperature. Experimental measurements give ln⁡K=−5.20\ln K = -5.20. A previously constructed ΔG∘\Delta G^{\circ} versus ln⁡K\ln K graph for this reaction yields a slope of −2.81 kJ-2.81\,\text{kJ} (units: kJ mol−1^{-1}). No ΔG∘\Delta G^{\circ} value was recorded at the time of measurement. (a) Calculate the numerical value of ΔG∘\Delta G^{\circ} for the reaction under these conditions. (b) Based on your result from part (a), discuss whether reactants or products are favored at equilibrium. (c) Determine the numerical value of the equilibrium constant KK and comment on how its magnitude supports your conclusion in part (b).

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