The gas-phase reaction below is studied at

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

Problem

The gas-phase reaction below is studied at 298 K298\,\text{K}, and the equilibrium constant is measured to be K=3.5×10−4K = 3.5 \times 10^{-4}. CO(g)+Cl2(g)⇌COCl2(g)CO(g) + Cl_2(g) \rightleftharpoons COCl_2(g) (1) Part 1: Determine the sign (positive, negative, or zero) of the standard free-energy change, ΔG∘\Delta G^\circ, for the reaction at 298 K298\,\text{K}. Explain your reasoning. (2) Part 2: Compare the magnitude of ∣ΔG∘∣|\Delta G^\circ| to RTRT at 298 K298\,\text{K} (assume R=8.314 J mol−1 K−1R = 8.314\,\text{J mol}^{-1}\,\text{K}^{-1}). State whether ∣ΔG∘∣|\Delta G^\circ| is much larger than, approximately equal to, or much smaller than RTRT, and justify your conclusion without performing an exact calculation. (3) Part 3: For the reverse reaction, predict whether it is thermodynamically favored under standard conditions. Support your prediction by referencing the relationship between ΔG∘\Delta G^\circ and KK.

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