(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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Class 11

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States of Matter

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Ideal gas equation and Related gas laws

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$A$ gas occupies a volume of $300 \ mL$ at $27 \ ^oC$ temperature and $730 \ mm$ pressure. What will be its volume at $STP$ in $mL$ (in $.2$)?

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What is the density of $SO_2$ gas at $27\,^oC$ temperature and $2\, atm$ pressure in $g/L$? (Atomic weights: $S = 32, O = 16, R = 0.082\, L\, atm\, K^{-1}\, mol^{-1}$)

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An open flask at $27^{\circ}C$ contains air. To what temperature $(^{\circ}C)$ should it be heated so that one-third of the air is expelled from the flask?

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$A$ sample of gas occupies $100 \ mL$ at $27 \ ^oC$ and $740 \ mm$ pressure. What will be the temperature of the gas in $^oC$ if its volume is changed to $80 \ mL$ at $740 \ mm$ pressure?

Medium

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At $25 \, ^\circ C$,the density of oxygen gas is $1.458 \, mg/L$ at $1 \, atm$ pressure. What will be the pressure of oxygen gas if the density is doubled?

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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

$A$ gas occupies a volume of $300 \ mL$ at $27 \ ^oC$ temperature and $730 \ mm$ pressure. What will be its volume at $STP$ in $mL$ (in $.2$)?

What is the density of $SO_2$ gas at $27\,^oC$ temperature and $2\, atm$ pressure in $g/L$? (Atomic weights: $S = 32, O = 16, R = 0.082\, L\, atm\, K^{-1}\, mol^{-1}$)

An open flask at $27^{\circ}C$ contains air. To what temperature $(^{\circ}C)$ should it be heated so that one-third of the air is expelled from the flask?

$A$ sample of gas occupies $100 \ mL$ at $27 \ ^oC$ and $740 \ mm$ pressure. What will be the temperature of the gas in $^oC$ if its volume is changed to $80 \ mL$ at $740 \ mm$ pressure?

At $25 \, ^\circ C$,the density of oxygen gas is $1.458 \, mg/L$ at $1 \, atm$ pressure. What will be the pressure of oxygen gas if the density is doubled?

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