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Gay Lussac's Law, Avagadro's Law

If excess wat...

Question

If excess water is added into a $100 g$ bottle sample labelled as $112 %$ $H_{2} S O_{4}$ and is reacted with $5.3 g N a_{2} C O_{3}$ , find the volume of $C O_{2}$ evolved at $1$ atm pressure and $300 K$ temperature after the completion of the reaction:

$H_{2} S O_{4} + N a_{2} C O_{3} \to N a_{2} S O_{4} + H_{2} O + C O_{2}$

$[R = 0.0821 L a t m m o l^{- 1} K^{- 1}]$

2.46 L

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24.6 L

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1.23 L

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12.3 L

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Solution

The correct option is C $1.23 L$
$1$ mole of sodium carbonate produces $1$ mole of carbon dioxide.

The number of moles of carbon dioxide produced from $5.3 g$ of sodium carbonate is $\frac{5.3}{106} = 0.05 m o l e s$ .

At $1$ atm pressure and $300 K$ temperature, $1$ mole of carbon dioxide occupies a volume of $24.63 L$ .

Volume of carbon dioxide produced from $5.3 g$ of sodium carbonate is $= 0.05 \times 24.63 = 1.23 L$ .

Hence, option C is correct.

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Similar questions

100 g

" 112 % H_{2} S O_{4} "

5.3 g

N a_{2} C O_{3}

C O_{2}

R = 0.0821 L a t m m o l

^{- 1} K^{- 1}

H_{2} S O_{4} + N a_{2} C O_{3} \to N a_{2} S O_{4} + H_{2} O + C O_{2}

112 % H_{2} S O_{4}

5.3

N a_{2} C O_{3}

C O_{2}

1

300

100 g

" 112 % H_{2} S O_{4} "

5.3 g

N a_{2} C O_{3}

C O_{2}

R = 0.0821 L a t m m o l

^{- 1} K^{- 1}

H_{2} S O_{4} + N a_{2} C O_{3} \to N a_{2} S O_{4} + H_{2} O + C O_{2}

100 g

112 %

H_{2} S O_{4}

5.3 g

N a_{2} C O_{3}

C O_{2}

300 K

H_{2} S O_{4} + N a_{2} C O_{3} \to N a_{2} S O_{4} + H_{2} O + C O_{2}

100 g

112 %

H_{2} S O_{4}

5.3 g

N a_{2} C O_{3}

C O_{2}

300 K

H_{2} S O_{4} + N a_{2} C O_{3} \to N a_{2} S O_{4} + H_{2} O + C O_{2}

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