Use the van der Waals equation for real gases to calculate the pressure exerted by 1.00 mole of ammonia at 27$\degree$C in a 750-mL container. (a = 4.17 L²*atm/mol², b = 0.0371 L/mol)

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The van der Waals equation is:$$P = \frac{nRT}{V - nb} - \frac{a}{V^2}$$where:P is the pressure in atmn is the number of moles of gasR is the ideal gas constant (0.0821 L*atm/mol*K)T is the temperature in KelvinV is the volume of the gas in La and b are the van der Waals constantsSubstituting the given values into the equation:$$P = \frac{(1.00 \text{ mol})(0.0821 \text{ L*atm/mol*K})(300 \text{ K})}{0.750 \text{ L} - (1.00 \text{ mol})(0.0371 \text{ L/mol})} - \frac{4.17 \text{ L}^2*\text{atm/mol}^2}{(0.750 \text{ L})^2}$$$$P = 27.1 \text{ atm}$$Therefore, the pressure exerted by 1.00 mole of ammonia at 27$\degree$C in a 750-mL container is 27.1 atm.

Use the Van Der Waals Equation for Real Gases to Calculate