Use the van der waals equation to calculate the pressure exerted by 1.335 mol of cl2 in a volume of 4.920 l at a temperature of 272.0 k.

Question

Dwayne Villanueva

Chemistry

22 December, 05:42

Use the van der waals equation to calculate the pressure exerted by 1.335 mol of cl2 in a volume of 4.920 l at a temperature of 272.0 k.

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Marlene Coleman · Answer 1

Van der waal or ideal eqn is given by PV = NRT; P = NRT / V. Where N = 1.335 is the number of moles. T = 272K is temperature. V = 4.920L is the volume. And R = 0.08205L. Substiting the values into the eqn; we have, P = (1.331 * 0.08205 * 272) / 4.920 = 29.7047 / 4.920 = 6.03atm.