One mole of an ideal gas at 1.00 bar sits in a cylinder in a large water bath at 300 K. The external pressure on the piston is suddenly raised to 5.00 bar and held there, and the gas is squeezed until its pressure is 5.00 bar, ending at 300 K. Take R = 8.314 J K⁻¹ mol⁻¹ and 1 L bar = 100 J. What is the total entropy change of the gas and the water bath?

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

One mole of an ideal gas at $1.00\ \text{bar}$ sits in a cylinder in a large water bath at $300\ \text{K}$ . The external pressure on the piston is suddenly raised to $5.00\ \text{bar}$ and held there, and the gas is squeezed until its pressure is $5.00\ \text{bar}$ , ending at $300\ \text{K}$ . Take $R = 8.314\ \text{J K}^{-1}\ \text{mol}^{-1}$ and $1\ \text{L bar} = 100\ \text{J}$ . What is the total entropy change of the gas and the water bath?

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