Four reactions have the values of Δ H° and Δ S° given below, which may be taken as constant with temperature. Which reaction is not spontaneous under standard conditions at 298 K but becomes spontaneous at 1000 K?

ChemistryHardHigh School (11–12)Chemical Thermodynamics › Entropy, Gibbs Energy and Spontaneity JEE Main JEE Advanced

Four reactions have the values of $\Delta H^\circ$ and $\Delta S^\circ$ given below, which may be taken as constant with temperature. Which reaction is not spontaneous under standard conditions at $298\ \text{K}$ but becomes spontaneous at $1000\ \text{K}$ ?

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← For the gas-phase isomerisation A(g) ⇌ B(g), Δ H° = -10.0 kJ mol⁻¹ and Δ S° = -16.0 J K⁻¹ mol⁻¹. Take R = 8.314 J K⁻¹ mol⁻¹ and Δ G° = -2.303 RT log K. What is the equilibrium constant K at 298 K, to the nearest integer?One mole of liquid benzene boils at its boiling point, 353.2 K, under a constant pressure of 1 bar. The enthalpy of vaporisation is 30.8 kJ mol⁻¹. Treat the vapour as an ideal gas and neglect the volume of the liquid. With w the work done on the system (R = 8.314 J K⁻¹ mol⁻¹), which pair of values is correct? →

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