(D) Initial state for gas $A$: $P_1 = 8 \ atm$, $V_1 = 12 \ L$. Total volume after opening the stop cock: $V_{total} = 12 \ L + 8 \ L = 20 \ L$.Since

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(D) Initial state for gas $A$: $P_1 = 8 \ atm$, $V_1 = 12 \ L$. Total volume after opening the stop cock: $V_{total} = 12 \ L + 8 \ L = 20 \ L$.Since the temperature is constant, we use Boyle's Law $(P_1V_1 = P_2V_2)$ for each gas independently.For gas $A$: $8 \ atm \times 12 \ L = P_A \times 20 \ L \implies P_A = \frac{96}{20} = 4.8 \ atm$.For gas $B$: $5 \ atm \times 8 \ L = P_B \times 20 \ L \implies P_B = \frac{40}{20} = 2.0 \ atm$.Thus, the partial pressures of $A$ and $B$ are $4.8 \ atm$ and $2.0 \ atm$ respectively.

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

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Two vessels are filled with ideal gases $A$ and $B$ and are connected through a pipe of zero volume as shown in the figure. The stop cock is opened and the gases are allowed to mix homogeneously and the temperature is kept constant. The partial pressures of $A$ and $B$ respectively (in $atm$) are:

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A
$8.0, 5.0$
B
$9.6, 4.0$
C
$6.4, 4.0$
D
$4.8, 2.0$

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Class 11

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States of Matter

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Ideal gas equation and Related gas laws

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At $300\, K$,the density of a certain gaseous molecule at $2\, bar$ is double that of dinitrogen $(N_2)$ at $4\, bar$. The molar mass of the gaseous molecule is ............... $g\, mol^{-1}$.

DifficultJEE MAIN 2017

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At temperature $T$,$1$ mole of $O_2$ gas (molar mass $32 \ g/mol$) is present in a container,exerting a pressure $P$. If $1$ mole of $He$ gas (molar mass $4 \ g/mol$) is placed in an identical container at temperature $2T$,what will be the pressure exerted by the $He$ gas?

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The equation for Boyle's law is:

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At $27\,^oC$ temperature in a $2\, L$ closed vessel,$10\, g$ of $H_2$ and $22\, g$ of $CO_2$ gases are filled. Find the partial pressure of each gas and the total pressure of the mixture. (Use $R = 0.08314\, L \cdot bar \cdot K^{-1} \cdot mol^{-1}$ and formula $pV = nRT$)

Difficult

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Calculate the new volume of a gas at constant pressure when temperature is increased to $546 \ K$.
[Initial volume of a gas at $273 \ K$ is $4 \ dm^3$] (in $dm^3$)

MediumMHT CET 2022

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Two vessels are filled with ideal gases $A$ and $B$ and are connected through a pipe of zero volume as shown in the figure. The stop cock is opened and the gases are allowed to mix homogeneously and the temperature is kept constant. The partial pressures of $A$ and $B$ respectively (in $atm$) are:

Similar Questions

At $300\, K$,the density of a certain gaseous molecule at $2\, bar$ is double that of dinitrogen $(N_2)$ at $4\, bar$. The molar mass of the gaseous molecule is ............... $g\, mol^{-1}$.

At temperature $T$,$1$ mole of $O_2$ gas (molar mass $32 \ g/mol$) is present in a container,exerting a pressure $P$. If $1$ mole of $He$ gas (molar mass $4 \ g/mol$) is placed in an identical container at temperature $2T$,what will be the pressure exerted by the $He$ gas?

The equation for Boyle's law is:

At $27\,^oC$ temperature in a $2\, L$ closed vessel,$10\, g$ of $H_2$ and $22\, g$ of $CO_2$ gases are filled. Find the partial pressure of each gas and the total pressure of the mixture. (Use $R = 0.08314\, L \cdot bar \cdot K^{-1} \cdot mol^{-1}$ and formula $pV = nRT$)

Calculate the new volume of a gas at constant pressure when temperature is increased to $546 \ K$. [Initial volume of a gas at $273 \ K$ is $4 \ dm^3$] (in $dm^3$)

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Calculate the new volume of a gas at constant pressure when temperature is increased to $546 \ K$.
[Initial volume of a gas at $273 \ K$ is $4 \ dm^3$] (in $dm^3$)