A mixture of and has a density of 1.5 g/l at 27°C and 760 mm pressure. If 1 l of the mixture is exposed to alkali, what would be the pressure of the remaining gas at the same volume and temperature?

Question

A mixture of $CO$ and $CO_2$ has a density of 1.5 g/l at 27°C and 760 mm pressure. If 1 l of the mixture is exposed to alkali, what would be the pressure of the remaining gas at the same volume and temperature?

Prashant Kotian · Accepted Answer

Correct answer: C. density d = 1.5 g/l, t = 300 k, p = 1 atm. from d = p × m_avg / (r × t) → 1.5 = 1 × m_avg / (0.0821 × 300) → m_avg = 36.95 g/mol. let mole fraction of co2 be x. m_avg = x × 44 + (1 - x) × 28 = 28 + 16x = 36.95 → 16x = 8.95 → x = 0.559. mole fraction of co = 1 - 0.559 = 0.441. alkali absorbs co2 completely. the remaining gas is co. since volume and temperature are constant, the final pressure equals the partial pressure of co: p_co = 0.441 × 760 mm hg = 335 mm hg.

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