A and B are ideal gases. The molecular weight | vedclass

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Question

(A) Let the weight of both gases $A$ and $B$ be $w \ g$. Given molecular weight ratio $M_A : M_B = 1 : 4$. Let $M_A = x$ and $M_B = 4x$. Moles of $A$

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$\frac{P}{5}$

Vedclass · Answer

(A) Let the weight of both gases $A$ and $B$ be $w \ g$. Given molecular weight ratio $M_A : M_B = 1 : 4$. Let $M_A = x$ and $M_B = 4x$. Moles of $A$ $(n_A)$ $= \frac{w}{x}$. Moles of $B$ $(n_B)$ $= \frac{w}{4x}$. Mole ratio $n_A : n_B = \frac{w}{x} : \frac{w}{4x} = 4 : 1$. Partial pressure of $B$ $(p_B)$ $= 	ext{Mole fraction of } B 	imes P_{total}$. $p_B = \frac{n_B}{n_A + n_B} 	imes P = \frac{1}{4 + 1} 	imes P = \frac{P}{5} \ atm$.

$A$ 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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