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Standard XII

Chemistry

Enthalpy of Combustion

Minimum amoun...

Question

Minimum amount of $A g_{2} C O_{3}$ (s) required to produce sufficient oxygen for the compelete combusion of $C_{2} H_{2}$ which produces $11.2 l t r$ of $C O_{2}$ at S.T.P after combusion is : [Ag =108]
$A g_{2} C O_{3} (s) \to 2 A g (s) + C O_{2} (g) + 1 / 2 o_{2} (g)$
$C_{2} H_{2} + 5 / 2 O_{2} \to 2 C O_{2} + H_{2} O$

276 g

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345 g

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690 g

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1380 g

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Solution

The correct option is B $345 g$
${A g_{2} C O_{3}}_{(s)} ⟶ {2 A g}_{(s)} + {C O_{2}}_{(g)} + {\frac{1}{2} O_{2}}_{(g)} ⟶ (1)$
$C_{2} H_{2} + \frac{5}{2} O_{2} ⟶ 2 C O_{2} + H_{2} O ⟶ (2)$
$11.2$ litre of $C O_{2}$ at STP= $\frac{11.2}{22.4} = 0.5$ mole of $C O_{2}$
From equation $(2)$ , $2$ moles of $C O_{2}$ is produced from $2.5$ mole of $O_{2}$ .
$∴ 0.5$ mole of $C O_{2}$ will be formed from= $\frac{2.5}{2} \times 0.5 = 0.625$ mole of $O_{2}$
Now, $1$ mole of $A g_{2} C O_{3}$ (equation 1) produces $0.5$ mole of $O_{2}$
$0.625$ mole of $O_{2}$ is formed from= $0.625 \times 2 = 1.25$ mole of $A g_{2} C O_{3}$ .
Molar mass of $A g_{2} C O_{3} = 276 g m m o l^{- 1}$
$∴$ Minimum amount of $A g_{2} C O_{3} = 276 \times 1.25 g m = 345 g m$

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Similar questions

The minimum amount of $A g_{2} C O_{3} (s)$ required to produce sufficient oxygen for the complete combustion of $C_{2} H_{2}$ , which produces $11.2 L$ of $C O_{2}$ at STP after combustion is: $[A g = 108]$

$A g_{2} C O_{3} (s) \to 2 A g (s) + C O_{2} (g) + \frac{1}{2} O_{2} (g)$

$C_{2} H_{2} + \frac{5}{2} O_{2} \to 2 C O_{2} + H_{2} O$

Q. The minimum amount of

A g_{2} C O_{3} (s)

required to produce sufficient oxygen for the complete combustion of

C_{2} H_{2}

, which produces

11.2 L

C O_{2}

at STP after combustion is:

[A g = 108]

A g_{2} C O_{3} (s) \to 2 A g (s) + C O_{2} (g) + \frac{1}{2} O_{2} (g)

C_{2} H_{2} + \frac{5}{2} O_{2} \to 2 C O_{2} + H_{2} O

Q. The minimum amount of

A g_{2} C O_{3} (s)

required to produce sufficient oxygen for the complete combustion of

C_{2} H_{2}

which produces

11.2 L

C O_{2}

at STP after combustion is:
(Molar mass of

A g = 108 g/mol

)

A g_{2} C O_{3 (s)} \to 2 A g_{(s)} + C O_{2 (g)} + \frac{1}{2} O_{2 (g)}

C_{2} H_{2} + \frac{5}{2} O_{2} \to 2 C O_{2} + H_{2} O

Q. Minimum amount of

A g_{2} C O_{3}

(s) required to produce sufficient amount of oxygen for the complete combustion of

C_{2} H_{2}

which produces 11.2 L of

C O_{2}

at STP after combustion is_________.

A g_{2} C O_{3} (s) \to 2 A g (s) + C O_{2} (g) + \frac{1}{2} O_{2} (g)

C_{2} H_{2} + \frac{5}{2} O_{2} \to 2 C O_{2} + H_{2} O

Q. The minimum amount of

A g_{2} C O_{3} (s)

required to produce sufficient oxygen for the complete combustion of

C_{2} H_{2}

which produces

11.2 L

C O_{2}

at STP after combustion is:
(Molar mass of

A g = 108 g/mol

)

A g_{2} C O_{3 (s)} \to 2 A g_{(s)} + C O_{2 (g)} + \frac{1}{2} O_{2 (g)}

C_{2} H_{2} + \frac{5}{2} O_{2} \to 2 C O_{2} + H_{2} O

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Minimum amount of Ag2CO3 (s) required to produce sufficient oxygen for the compelete combusion of C2H2 which produces 11.2ltr of CO2 at S.T.P after combusion is : [Ag =108]Ag2CO3(s)→2Ag(s)+CO2(g)+1/2o2(g)C2H2+5/2O2→2CO2+H2O