(A) The ideal gas equation is given by $PV = nRT$. Since $n = \frac{m}{M}$ and density $d = \frac{m}{V}$,we can write $P = \frac{dRT}{M}$. Given: $d =

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(A) The ideal gas equation is given by $PV = nRT$. Since $n = \frac{m}{M}$ and density $d = \frac{m}{V}$,we can write $P = \frac{dRT}{M}$. Given: $d = 8 \, kg \, m^{-3}$,$T = -40 + 273.15 = 233.15 \, K$,$R = 8.314 \, J \, K^{-1} \, mol^{-1}$,and $M = 0.0365 \, kg \, mol^{-1}$. Substituting the values: $P = \frac{8 \times 8.314 \times 233.15}{0.0365} \, Pa$. $P = \frac{15511.45}{0.0365} \, Pa \approx 4.25 \times 10^{5} \, Pa$.

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

Medium

Calculate the pressure of $HCl$ gas having a density of $8 \, kg \, m^{-3}$ at a temperature of $-40 \, ^oC$. (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$,Molar mass of $HCl = 36.5 \, g \, mol^{-1} = 0.0365 \, kg \, mol^{-1}$)

A
$4.24 \times 10^{5} \, Pa$
B
$5.24 \times 10^{5} \, Pa$
C
$3.24 \times 10^{5} \, Pa$
D
$6.24 \times 10^{5} \, Pa$

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Class 11

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States of Matter

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Ideal gas equation and Related gas laws

The density of a gas $A$ is three times that of a gas $B$. If the molecular mass of $A$ is $M$,the molecular mass of $B$ is:

Easy

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Two closed bulbs of equal volume $V$ containing an ideal gas initially at pressure $P_i$ and temperature $T_1$ are connected through a narrow tube of negligible volume as shown in the figure below. The temperature of one of the bulbs is then raised to $T_2$. The final pressure $P_f$ is:

DifficultJEE MAIN 2016

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$n$ moles of an ideal gas at temperature $T$ (in kelvin) occupy $V \ L$ of volume,exerting a pressure of $P$ atmospheres. What is the concentration (in $mol / L$)?

MediumAP EAMCET 2001

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$A$ container is divided into two equal parts $A$ and $B$ containing $H_2$ and $O_2$ respectively,each at $1 \ atm$ pressure. If the wall separating the two sections is removed,what happens to the pressure?

Medium

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If the density of dioxygen gas at $STP$ is $1.43 \, g \, L^{-1}$,calculate its density at $17 \, ^\circ C$ and $800 \, torr$ pressure.

Medium

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Calculate the pressure of $HCl$ gas having a density of $8 \, kg \, m^{-3}$ at a temperature of $-40 \, ^oC$. (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$,Molar mass of $HCl = 36.5 \, g \, mol^{-1} = 0.0365 \, kg \, mol^{-1}$)

Similar Questions

The density of a gas $A$ is three times that of a gas $B$. If the molecular mass of $A$ is $M$,the molecular mass of $B$ is:

Two closed bulbs of equal volume $V$ containing an ideal gas initially at pressure $P_i$ and temperature $T_1$ are connected through a narrow tube of negligible volume as shown in the figure below. The temperature of one of the bulbs is then raised to $T_2$. The final pressure $P_f$ is:

$n$ moles of an ideal gas at temperature $T$ (in kelvin) occupy $V \ L$ of volume,exerting a pressure of $P$ atmospheres. What is the concentration (in $mol / L$)?

$A$ container is divided into two equal parts $A$ and $B$ containing $H_2$ and $O_2$ respectively,each at $1 \ atm$ pressure. If the wall separating the two sections is removed,what happens to the pressure?

If the density of dioxygen gas at $STP$ is $1.43 \, g \, L^{-1}$,calculate its density at $17 \, ^\circ C$ and $800 \, torr$ pressure.

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