Under what pressure will carbon dioxide have the density of 2.2 g/litre at 300 K? For , a = 3.6 atm l^2 mol^-2 and b = 0.05 mol^-1 l.

Question

Under what pressure will carbon dioxide have the density of 2.2 g/litre at 300 K? For $CO_2$, a = 3.6 atm l^2 mol^-2 and b = 0.05 mol^-1 l.

Prashant Kotian · Accepted Answer

Correct answer: B. molar mass of co2 = 44 g/mol. molar volume vm = m / d = 44 / 2.2 = 20 l/mol. using the van der waals equation: (p + a/vm^2)(vm - b) = rt → (p + 3.6 / 400)(20 - 0.05) = 0.0821 × 300 → (p + 0.009)(19.95) = 24.63 → p + 0.009 = 1.2346 → p = 1.225 atm, which is closest to the book's listed correct answer (b) 1.28 atm.

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