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?

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

For the gas-phase isomerisation $\text{A}(g) \rightleftharpoons \text{B}(g)$ , $\Delta H^\circ = -10.0\ \text{kJ mol}^{-1}$ and $\Delta S^\circ = -16.0\ \text{J K}^{-1}\ \text{mol}^{-1}$ . Take $R = 8.314\ \text{J K}^{-1}\ \text{mol}^{-1}$ and $\Delta G^\circ = -2.303\,RT\log K$ . What is the equilibrium constant $K$ at $298\ \text{K}$ , to the nearest integer?

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← A sample of 2.00 mol of an ideal gas at 300 K is in a flask of 10 L. The flask sits inside a rigid, insulated box whose whole inside volume, flask included, is 50 L; the rest of the box is empty. The flask breaks and the gas fills the whole box. Take R = 8.314 J K⁻¹ mol⁻¹. What is the total entropy change of the gas and its surroundings together?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? →

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