When the pressure of a sample of gas is increased from 0.50 to 100 atm at constant temperature, its volume decreases from 2.0 l to 13 ml. What could cause the deviation from Boyle's law?

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Boyle's law predicts V = (0.50 × 2.0)/100 = 0.010 l = 10 ml at 100 atm; the observed volume is 13 ml, larger than ideal, i.e. Z > 1 at high pressure. A positive deviation at high pressure arises because the finite volume of the molecules themselves is a significant fraction of the container volume there. Ans: (a)

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