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Standard XI

Chemistry

Balancing Redox Equations

Water is adde...

Question

Water is added in excess to a $100 g$ sample labelled as $112 %$ $H_{2} S O_{4}$ This solution is then treated with $5.3 g$ of $N a_{2} C O_{3}$ . the volume of $C O_{2}$ evolved at 1atm and $300 K$ after a complete reaction will be :
$H_{2} S O_{4} + N a_{2} C O_{3} \to N a_{2} S O_{4} + H_{2} O + C O_{2}$

2.46 L

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24.60 L

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1.27 L

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12.30 L

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Solution

The correct option is C 1.27 L
$112 %$ $H_{2} S O_{4}$ means water is in excess and the mass of $H_{2} S O_{4}$ 112 g
Reaction :
$H_{2} S O_{4} + N a_{2} C O_{3} \to N a_{S} O_{4} + C O_{2} + H_{2} O$
number of mole of $H_{2} S O_{4} = 112 / 98$
number of mole of $N a_{2} C O_{3} = 5.3 / 106 = 0.05$
$N a_{2} C O_{3}$ is limiting reagent so 0.05 moles of $C O_{2}$ produced at STP which volume is eqaul to 1.27 L

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Similar questions

Q. Water is added in excess to a

100 g

sample labelled as

112 %

H_{2} S O_{4}

This solution is then treated with

5.3 g

N a_{2} C O_{3}

. the volume of

C O_{2}

evolved at 1atm and

300 K

after a complete reaction will be :

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

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 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.

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}

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}]

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Water is added in excess to a 100 g sample labelled as 112% H2SO4 This solution is then treated with 5.3 g of Na2CO3. the volume of CO2 evolved at 1atm and 300 K after a complete reaction will be : H2SO4+Na2CO3→Na2SO4+H2O+CO2

The correct option is C 1.27 L112% H2SO4 means water is in excess and the mass of H2SO4 112 g Reaction : H2SO4+Na2CO3→NaSO4+CO2+H2O number of mole of H2SO4=112/98 number of mole of Na2CO3=5.3/106=0.05 Na2CO3 is limiting reagent so 0.05 moles of CO2 produced at STP which volume is eqaul to 1.27 L