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Dalton's Law of Partial Pressures

A and B are...

Question

$A$ and $B$ are ideal gases. The molecular weights of $A$ and $B$ are in the ratio of 1: 4. The pressure of a gas mixture containing equal weights of $A$ and $B$ is $P$ $a t m$ . What is the partial pressure (in $a t m$ ) of $B$ in the mixture.

\frac{P}{5}

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\frac{P}{2}

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\frac{P}{2.5}

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\frac{3 P}{4}

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Solution

The correct option is B $\frac{P}{5}$
$P_{B} = P . X_{B}$
No. of moles of gas is inversely proportional to molecular weight when an equal mass of gases are present.
Thus, no. of moles of $A$ and $B$ are in the ratio 4: 1
Mole fraction of $B$ $= 1 / 5$
Thus, $P_{B} = \frac{P}{5}$

So, the correct option is $A$

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A and B are ideal gases. The molecular weights of A and B are in the ratio of 1: 4. The pressure of a gas mixture containing equal weights of A and B is P atm. What is the partial pressure (in atm) of B in the mixture.

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$A$ and $B$ are ideal gases. The molecular weights of $A$ and $B$ are in the ratio of 1: 4. The pressure of a gas mixture containing equal weights of $A$ and $B$ is $P$ $a t m$ . What is the partial pressure (in $a t m$ ) of $B$ in the mixture.