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A 82.1 L container connected with manometer contains mixture of ${CS}_{2}$ and $H_{2} S$ gases and added with required amount of oxygen to form to ${CO}_{2}, {SO}_{2}$ and $H_{2} O$ (g) at 227° C. Final conditions of manometer is shown. If moles of ${SO}_{2}$ gas produced is 0.7, with reference to above question select correct statement(s).

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Moles of ${CS}_{2}$ originally present is 0.3

Total pressure after combustion is 0.6atm

Moles of ${CS}_{2}$ originally present is 0.2

Moles of $H_{2} S$ originally present is 0.3

answer is B, C, D.

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Detailed Solution

$\begin{array}{l} P = 1 - \frac{304}{760} = 0.6 atm \\ 0.6 \times 82.1 = n \times 0.0821 \times 500 \end{array}$

Total moles of gas = 1.2

$\underset{x mole}{{CS}_{2}} + O_{2} ⟶ \underset{x}{{CO}_{2}} + \underset{2 x}{2 {SO}_{2}}$

$\underset{y}{H_{2} S} + O_{2} ⟶ \underset{y}{H_{2} O} + \underset{y}{{SO}_{2}}$

$\begin{array}{l} 3 x + 2 y = 1.2 \\ (2 x + y) \times 2 = \frac{700}{1000} \times 2 \\ 2 x + y = 0.7 \\ x = 0.2 \\ y = 0.3 \end{array}$

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