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Molecular Formula

Minimum amoun...

Question

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_________.
$A g_{2} C O_{3} (s) \to 2 A g (s) + C O_{2} (g) + \frac{1}{2} O_{2} (g)$
$C_{2} H_{2} + \frac{5}{2} O_{2} \to 2 C O_{2} + H_{2} O$

A

276

g

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B

345

g

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C

690

g

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D

1380

g

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Solution

The correct option is B $345$ g
11.2 L of $C O_{2}$ at STP $= \frac{11.2 L}{22.4 L/mol} = 0.5 mol$
$2 moles$ of $C O_{2} = \frac{5}{2}$ moles of $O_{2}$ required for the complete combustion of $C_{2} H_{2}$ .
$1 mole$ of $C O_{2} = \frac{5}{2 \times 2}$ moles of $O_{2}$ required for the complete combustion of $C_{2} H_{2}$ .
$0.5 mol$ of $C O_{2} = 0.5 mol \times \frac{5}{2 \times 2} = \frac{5}{8}$ moles of $O_{2}$ required for the complete combustion of $C_{2} H_{2}$ .
$\frac{1}{2}$ moles of $O_{2}$ $= 1$ mole of $A g_{2} C O_{3} (s)$ required.
$1$ moles of $O_{2}$ $= 2$ mole of $A g_{2} C O_{3} (s)$ required.
$\frac{5}{8}$ moles of $O_{2}$ $= 2 \times \frac{5}{8} = \frac{5}{4}$ moles of $A g_{2} C O_{3} (s)$ required.
The molar mass of $A g_{2} C O_{3} (s) = 275.75$ g/mol.
The mass of $A g_{2} C O_{3} (s)$ required $= 275.75$ g/mol $\times \frac{5}{4}$ mol $= 345$ g.

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Similar questions

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}

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. 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

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}

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 oxygen for the compelete combusion of

C_{2} H_{2}

11.2 l t r

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

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