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Standard XII

Chemistry

Haber Bosch Process

If excess wat...

Question

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

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 $1.23 L$
The reaction is as follows:
$N a_{2} C O_{3} + H_{2} S O_{4} \to N a_{2} S O_{4} + H_{2} O + C O_{2}$
Moles of $C O_{2}$ formed $=$ Moles of $N a_{2} C O_{3}$ reacted $= \frac{5.3}{106} = 0.05$ .
Volume of $C O_{2}$ formed at $1$ atm pressure and $300 K = 0.05 \times 24.63 = 1.23 L$ .

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Similar questions

Q. If excess water is added into a bottle sample labelled as

112 %

H_{2} {S O}_{4}

and is reacted with

5.3

{N a}_{2} {C O}_{3}

, then find the volume of

{C O}_{2}

evolved at

1

atm pressure and

300

K temperature after the completion of the reaction.

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}]

Q. 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}

, then find the volume of

C O_{2}

evolved at STP after the completion of the reaction : [

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}

Q. 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.

Q. 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}

, then find the volume of

C O_{2}

evolved at STP after the completion of the reaction : [

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}

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If excess water is added into a bottle sample labelled as 112%H2SO4 and is reacted with 5.3 g Na2CO3, then find the volume of CO2 evolved at 1 atm pressure and 300 K temperature after the completion of the reaction.

The correct option is C 1.23LThe reaction is as follows:Na2CO3+H2SO4→Na2SO4+H2O+CO2Moles of CO2 formed = Moles of Na2CO3 reacted=5.3106=0.05.Volume of CO2 formed at 1 atm pressure and 300K=0.05×24.63=1.23L.

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