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Standard XII

Chemistry

Order of Reaction

A 100 g pur...

Question

A $100 g$ pure sample of $N a H C O_{3}$ was heated until $11.2 L$ of $C O_{2} (g)$ was collected at $S T P$ . What percentage of the $N a H C O_{3}$ had decomposed?
$N a H C O_{3} (s) \to N a_{2} C O_{3} (s) + H_{2} O + C O_{2}$

50 %

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42 %

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84 %

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100 %

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Solution

The correct option is B $42 %$
moles of $C O_{2}$ formed $= \frac{11.2}{22.4} = 0.5$
$∵$ 1 mole of $N a H C O_{3}$ gives 1 mole of $C O_{2}$ .
$∴$ moles of $N a H C O_{3}$ decomposed $= 0.5$ .
$∴$ Weight of $N a H C O_{3}$ decomposed $= 0.5 \times 84 = 42 g$
$∴ %$ of $N a H C O_{3}$ decomposed $= \frac{42}{100} \times 100 = 42 %$

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Similar questions

Q. A 2 g sample containing

N a_{2} C O_{3}

and

N a H C O_{3}

loses 0.62 g when heated to

300^{o} C,

the temperature at which

N a H C O_{3}

decomposes to

N a_{2} C O_{3}, C O_{2}

and

H_{2} O .

What is the percentage of

N a_{2} C O_{3}

in the given mixture.

Q. A sample contains a mixture of

N a H C O_{3}

and

N a_{2} C O_{3}

H C l

is added to

15.0

g of the sample yielding

11.0

N a C l

. What percent of the sample is

N a_{2} C O_{3}

?
Reactions are:

N a_{2} C O_{3} + 2 H C l \to 2 N a C l + C O_{2} + H_{2} O

N a H C O_{3} + H C l \to N a C l + C O_{2} + H_{2} O

Molecular weight of

N a C l

N a H C O_{3}

and

N a_{2} C O_{3}

58.5

84

and

106

g/mol respectively.

Q. A

2.0

g sample containing

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

and

N a H C O_{3}

loses

0.248

g when heated to

300

^{o} C

, the temperature at which

N a H C O_{3}

decomposes to

{N a}_{2} C O_{3}, C O_{2}

and

H_{2} O

. The

%

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

in the mixture is (as the nearest integer):

4g of a mixture of Na₂CO₃and NaHCO₃ on heating liberates 448 mL of CO₂ at STP. The percentage of Na₂CO₃ in the mixture is?

Q. A mixture of

N a H C O_{3}

and

N a_{2} C O_{3}

weighed .0235 g. The dissolved mixture was reacted with excess of

8 a (O H)_{2}

to form

2.1028 g B a C O_{3}

, by the following reactions:

N a_{2} C O_{3} + B a (O H)_{2} \to B a C O_{3} + 2 N a O H

N a H C O_{3} + B a (O H)_{2} \to B a C O_{3} + N a O H + H_{2} O

What was the percentage of

N a H C O_{3}

in the original mixture ?

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A 100 g pure sample of NaHCO3 was heated until 11.2 L of CO2(g) was collected at STP. What percentage of the NaHCO3 had decomposed?NaHCO3(s)→Na2CO3(s)+H2O+CO2

The correct option is B 42%moles of CO2 formed=11.222.4=0.5∵ 1 mole of NaHCO3 gives 1 mole of CO2.∴ moles of NaHCO3 decomposed=0.5.∴ Weight of NaHCO3 decomposed=0.5×84=42g∴% of NaHCO3 decomposed=42100×100=42%

A $100 g$ pure sample of $N a H C O_{3}$ was heated until $11.2 L$ of $C O_{2} (g)$ was collected at $S T P$ . What percentage of the $N a H C O_{3}$ had decomposed?
$N a H C O_{3} (s) \to N a_{2} C O_{3} (s) + H_{2} O + C O_{2}$