20 ml of a mixture of CO and H₂ were mixed with excess of O₂ and exploded and cooled. There was a volume contraction of 18 mL. All volume measurements corresponds to room temperature (27°C) and one atmospheric pressure. Determine the volume ratioV₁:V₂ of CO and H₂ in the original mixture.

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1:2

3 : 2

2:3

4 : 1

answer is B.

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Detailed Solution

$\underset{x}{CO} + \underset{x / 2}{\frac{1}{2} O_{2}} ⟶ \underset{x}{{CO}_{2}}$
$\underset{(20 - x)}{H_{2}} + \underset{(\frac{20 - x}{2})}{\frac{1}{2} O_{2}} ⟶ H_{2} O (l); Volume contraction = V . R - V . P = (x + \frac{x}{2} - x) + [20 - x + \frac{1}{2} (20 - x) - 0] 18 = \frac{x}{2} + \frac{3 (20 - x)}{2}$
$\begin{array}{l} x = 12 mL = CO \\ H_{2} = 8 mL \\ V_{CO} : V_{H_{2}} = 12 : 8 = 3 : 2 \end{array}$