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

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

Class 11 Chemistry States of Matter Mix Examples- States of Matter

Medium

$A$ 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 $P \text{ atm}$. What is the partial pressure (in $\text{atm}$) of $B$ in the mixture?

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A
$\frac{P}{5}$
B
$\frac{P}{2}$
C
$\frac{P}{2.5}$
D
$\frac{3P}{4}$

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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 $P \text{ atm}$. What is the partial pressure (in $\text{atm}$) of $B$ in the mixture?

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