(B) Using the ideal gas equation $PV = nRT$,since $T$ is constant,$n = \frac{PV}{RT}$.For $CH_4$: $n_1 = \frac{2 \times 2}{RT} = \frac{4}{RT}$.For $CO

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(B) Using the ideal gas equation $PV = nRT$,since $T$ is constant,$n = \frac{PV}{RT}$.For $CH_4$: $n_1 = \frac{2 \times 2}{RT} = \frac{4}{RT}$.For $CO_2$: $n_2 = \frac{4 \times 3}{RT} = \frac{12}{RT}$.For $Ne$: $n_3 = \frac{3 \times 4}{RT} = \frac{12}{RT}$.Total moles $n_T = n_1 + n_2 + n_3 = \frac{4 + 12 + 12}{RT} = \frac{28}{RT}$.Total volume $V_T = 2 + 3 + 4 = 9 \ L$.Final pressure $P_T = \frac{n_T RT}{V_T} = \frac{28}{RT} \times \frac{RT}{9} = \frac{28}{9} \approx 3.11 \ atm$.The nearest integer is $3$.

Class 11 Chemistry States of Matter Ideal gas equation and Related gas laws

Medium

Three bulbs are filled with $CH_4$,$CO_2$,and $Ne$ as shown in the picture. The bulbs are connected through pipes of zero volume. When the stopcocks are opened and the temperature is kept constant throughout,the pressure of the system is found to be $...... \ atm$. (Nearest integer)

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A
$2$
B
$3$
C
$4$
D
$1$

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States of Matter

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Ideal gas equation and Related gas laws

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Three bulbs are filled with $CH_4$,$CO_2$,and $Ne$ as shown in the picture. The bulbs are connected through pipes of zero volume. When the stopcocks are opened and the temperature is kept constant throughout,the pressure of the system is found to be $...... \ atm$. (Nearest integer)

Similar Questions

At what temperature in $K$ will $28 \ g$ of $N_2$ gas occupy a volume of $10.0 \ L$ at $2.46 \ atm$ pressure?

If $10^{-4} \ dm^3$ of water is introduced into a $1.0 \ dm^3$ flask at $300 \ K,$ how many moles of water are in the vapour phase when equilibrium is established? (Given: Vapour pressure of $H_2O$ at $300 \ K$ is $3170 \ Pa;$ $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)

$A$ gas occupies $2.5 \ L$ at $0 \ ^oC$ and $1 \ atm$ pressure. If the pressure is increased to $1.5 \ atm$ and the gas is transferred to a $2.0 \ L$ container,what will be the change in temperature in $^oC$?

The volume versus temperature graph of $1 \ mole$ of an ideal gas is given below. The pressure of the gas (in $atm$) at $X, Y$ and $Z$,respectively,are

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