At very high pressures, the volume of a real gas is larger than that predicted by the ideal gas law because real molecules occupy space, which the ideal gas law neglects. At what pressure would the Van der Waals equation of state result in a volume that was 5% larger than that predicted by the ideal gas law for 1 mol of water vapor at a temperature of 0°C? Assume a = 0.546 Pa mб/mol2 and b = 3.05 x 10-5 m³/mol. Pa

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A: Please refer the attached image for complete solution.

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