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?

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

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

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← 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?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? →

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