For a gas-phase reaction, Δ G° = +10.0 kJ mol⁻¹ at 300 K and Δ G° = -5.0 kJ mol⁻¹ at 400 K. Taking Δ H° and Δ S° as constant over this range, at what temperature is the equilibrium constant of the reaction equal to 1?

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For a gas-phase reaction, $\Delta G^\circ = +10.0\ \text{kJ mol}^{-1}$ at $300\ \text{K}$ and $\Delta G^\circ = -5.0\ \text{kJ mol}^{-1}$ at $400\ \text{K}$ . Taking $\Delta H^\circ$ and $\Delta S^\circ$ as constant over this range, at what temperature is the equilibrium constant of the reaction equal to 1?

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← The standard enthalpy of formation of methane, CH₄(g), is -74.8 kJ mol⁻¹. The enthalpy of atomisation of graphite, C(graphite) → C(g), is 716.7 kJ mol⁻¹, and the bond enthalpy of H₂ is 435.8 kJ mol⁻¹. What is the mean C-H bond enthalpy in methane, in kJ mol⁻¹, to the nearest integer?An ideal gas is taken once round the cycle A to B to C to A shown in the figure. From A (10 L, 2.0 bar) it expands at constant pressure to B (30 L), then its pressure falls at constant volume to C (1.0 bar), and it returns to A along the straight line CA. Take 1 L bar = 100 J. How much heat q does the gas take in over one cycle? →

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