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Molarity

The pressure ...

Question

The pressure of $11$ gm of a gas which is placed in a $4$ litres container at $127^{0} C$ is $2$ atm, then the gas would be:

[Take $R = 0.08$ L atm/mol K]

N_{2} O

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O_{3}

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N O_{2}

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C O_{2}

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Solution

The correct options are
A $N_{2} O$
D $C O_{2}$
According to ideal gas equation, we have $P V = n R T$
We also know,

$N o . o f m o l e s (n) = \frac{M a s s (W)}{M o l a r m a s s (M)}$

Therefore, we can rewrite the ideal gas equation as:

$P V = \frac{W R T}{M}$

To identify the gas, we need to determine the molar mass (M).
$M = \frac{W R T}{P V}$

$= \frac{11 \times 0.08 \times 400}{2 \times 4} = 44 g m o l^{- 1}$

So, the molar mass of the unknown gas is $44 g m o l^{- 1}$

So, the unknown gas could be either $N_{2} O$ or $C O_{2}$ .
Hence, options $A$ and $D$ are correct.

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127^{o} C

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27^{\circ}

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