Two gaseous reactions are studied at constant pressure

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

Problem

Two gaseous reactions are studied at constant pressure. Their standard Gibbs free energy changes vary with temperature according to the following expressions (units: kJ\mathrm{kJ}; TT in K\mathrm{K}): Reaction A: ΔGA∘=40.0−0.10 T\Delta G^\circ_{A} = 40.0 - 0.10\,T Reaction B: ΔGB∘=−20.0+0.05 T\Delta G^\circ_{B} = -20.0 + 0.05\,T (a) Calculate the temperature at which the two reactions have the same standard Gibbs free energy change. (b) At 500 K500\,\text{K}, which reaction is thermodynamically favored (i.e., ΔG∘<0\Delta G^\circ < 0)?

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