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Introduction to Oxidation and Reduction

If excess wat...

Question

If excess water is added into a bottle labelled as $109 % H_{2} S O_{4}$ and is reacted with $6.6 g N a_{2} C O_{3}$ then find the volume of $C O_{2}$ evolved at $1 a t m$ and $273 K$ after the completion of the reaction.

A

22.4 L

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B

1.4 L

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C

2.2 L

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D

14.2 L

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Solution

The correct option is B $1.4 L$
$N a_{2} C O_{3} + H_{2} S O_{4} \to N a_{2} S O_{4} + H_{2} O + C O_{2}$

$Moles of N a_{2} C O_{3} = \frac{6.6 g}{106 g / m o l} \approx 0.0623 m o l$
According to the stoichiometry of the reaction,
$1 m o l N a_{2} C O_{3} \equiv 1 m o l C O_{2}$
$∴$ Moles of $C O_{2} = 0.0623 m o l$

From ideal gas equation,
$V = \frac{n R T}{P}$
$∴ V_{C O_{2}} = \frac{0.0623 m o l \times 0.0821 L a t m K^{- 1} m o l^{- 1} \times 273 K}{1 a t m}$
$V_{C O_{2}} \approx 1.4 L$

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Similar questions

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