(A) Using the ideal gas law $PV = nRT$,we find the moles of each gas at constant temperature $T = 300 \ K$.For $H_2$: $n_1 = \frac{P_1 V_1}{RT} = \fra

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(A) Using the ideal gas law $PV = nRT$,we find the moles of each gas at constant temperature $T = 300 \ K$.For $H_2$: $n_1 = \frac{P_1 V_1}{RT} = \frac{1 \ bar \times 1 \ L}{RT} = \frac{1}{RT}$.For $O_2$: $n_2 = \frac{P_2 V_2}{RT} = \frac{2 \ bar \times 2 \ L}{RT} = \frac{4}{RT}$.Total moles $n_{total} = n_1 + n_2 = \frac{1+4}{RT} = \frac{5}{RT}$.In the $10 \ L$ flask,the total pressure $P_{total}$ is given by $P_{total} = \frac{n_{total} RT}{V_{final}}$.$P_{total} = \frac{(5/RT) \times RT}{10 \ L} = \frac{5}{10} \ bar = 0.5 \ bar$.

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

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At $27^{\circ} C$,$1 \ L$ of $H_2$ with a pressure of $1 \ bar$ is mixed with $2 \ L$ of $O_2$ with a pressure of $2 \ bar$ in a $10 \ L$ flask. What is the pressure exerted by the gaseous mixture in $bar$? (Assume $H_2$ and $O_2$ as ideal gases)

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A
$0.5$
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$0.4$
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$1.0$
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$0.1$

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States of Matter

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Ideal gas equation and Related gas laws

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At $27^{\circ} C$,$1 \ L$ of $H_2$ with a pressure of $1 \ bar$ is mixed with $2 \ L$ of $O_2$ with a pressure of $2 \ bar$ in a $10 \ L$ flask. What is the pressure exerted by the gaseous mixture in $bar$? (Assume $H_2$ and $O_2$ as ideal gases)

Similar Questions

Find the number of moles of $CO_2$ present in a sample occupying $4 \times 10^{-3} \text{ m}^3$ at $1.104 \times 10^5 \text{ Nm}^{-2}$ pressure. Given: $R \times T = 2208 \text{ J mol}^{-1}$. (in $\text{ mole}$)

At $0\, ^\circ C$ and $1\, \text{atm}$ pressure,a gas occupies $100\, \text{cc}$. If the pressure is increased to $1.5$ times and the temperature is increased by one-third of its absolute temperature,then the final volume of the gas will be :- $cc$

If the density ratio of a gas is $1:2$ and the temperature ratio is $2:1$,what will be the ratio of their pressures?

$A$ gas has a volume of $3.4 \ L$ at $298 \ K$. What is the final temperature if the volume of gas increases to $6.8 \ L$ (in $K$)?

The pressure exerted by $6.0 \ g$ of methane gas in a $0.03 \ m^3$ vessel at $129 \ ^oC$ is : (Atomic masses of $C = 12.01, H = 1.01$ and $R = 8.314 \ J K^{-1} mol^{-1}$) :- ................ $Pa$

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