One mole of an ideal gas at 22.4L is expanded isothermally and reversibly at 300 K to a volume of 224 L at a constant pressure. Calculate the magnitude of ΔG in kJ. (Given, R=8.314J K−1 mol−1). Give your answer upto two decimal only)
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Solution
Given, n=1moleVi=22.4LVf=224LT=300K W=−2.303×nRTlogVfVi=−2.303×1×8.314×10−3×300×log22422.4=−2.303×2×0.3=−5.74kJ ΔG= work done in reversible process which is maximum work done =−5.74kJ