What is the molecular weight of a gas that has a density of $2 g / L$ at a temperature of $300 K$ and a pressure of $2 a t m$ ?

24.6 g / m o l

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22 g / m o l

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18 g / m o l

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26 g / m o l

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Solution

The correct option is A $24.6 g / m o l$
We know, $P V = n R T$

$n = m / M_{M} =$ number of moles

where, $m =$ mass and $M_{M} =$ molar mass

Thus, $P V = \frac{m}{M_{M}} R T$

$M_{M} = \frac{m}{V} \frac{R T}{P}$ where, $\frac{m}{V} = ρ =$ density

$M_{M} = ρ \frac{R T}{P}$

putting the values,

$M_{M} = 2 \times \frac{0.0821 \times 300}{2} = 24.6$ g/mol

Hence, the correct option is $A$ .

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A gas exerts a pressure of 0.892 atm in a 5.00 L container at 15º C. The density of the gas is 1.22 g/L. What is the molecular weight of the gas?

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1.6

a = 4.0

L^{2}

m o l^{- 2}

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= 0.08

R T = 25 l i t . a t m . m o l^{- 1}

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m o l^{- 1}

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