(C) Using the Ideal Gas Law: $PV = nRT$,where $n = \frac{m}{M}$.Here,$P = 22.4\,atm$,$V = 2\,L$,$T = 273\,K$,and the molar mass of $N_2$ is $M = 28\,g

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(C) Using the Ideal Gas Law: $PV = nRT$,where $n = \frac{m}{M}$.Here,$P = 22.4\,atm$,$V = 2\,L$,$T = 273\,K$,and the molar mass of $N_2$ is $M = 28\,g/mol$.The gas constant $R = 0.0821\,L \cdot atm \cdot K^{-1} \cdot mol^{-1}$.Substituting the values: $22.4 \times 2 = n \times 0.0821 \times 273$.Since $0.0821 \times 273 \approx 22.4$,we get $22.4 \times 2 = n \times 22.4$,which implies $n = 2\,mol$.The mass $m = n \times M = 2\,mol \times 28\,g/mol = 56\,g$.

Class 11 Physics Kinetic Theory of Gases Gas Laws (Charles, Boyle's, Avagadro's, Gay Lussacs and Dalton's law) and Ideal gas Equation

Medium

What is the mass of $2$ litres of nitrogen gas $(N_2)$ at $22.4$ atmospheric pressure and $273\,K$?

A
$28\,g$
B
$14 \times 22.4\,g$
C
$56\,g$
D
None of these

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Kinetic Theory of Gases

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Gas Laws (Charles, Boyle's, Avagadro's, Gay Lussacs and Dalton's law) and Ideal gas Equation

The expansion of unit mass of a perfect gas at constant pressure is shown in the diagram. Here

Medium

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Estimate the total number of air molecules (inclusive of oxygen,nitrogen,water vapour,and other constituents) in a room of capacity $25.0 \; m^{3}$ at a temperature of $27^{\circ} C$ and $1 \; atm$ pressure.

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$A$ gas has a volume of $251 \,cm^3$ at $20^{\circ} C$ and a pressure of $78 \,cm$ of $Hg$. Find its volume at $NTP$. (in $\,cm^3$)

MediumAP EAMCET 2020

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In the given $(V - T)$ diagram,what is the relation between pressures $P_1$ and $P_2 \,?$

MediumJEE MAIN 2022

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$A$ gas at $27^{\circ}C$ has a volume $V$ and pressure $P$. On heating,its pressure is doubled and volume becomes three times. The resulting temperature of the gas will be ...... $^{\circ}C$.

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What is the mass of $2$ litres of nitrogen gas $(N_2)$ at $22.4$ atmospheric pressure and $273\,K$?

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The expansion of unit mass of a perfect gas at constant pressure is shown in the diagram. Here

Estimate the total number of air molecules (inclusive of oxygen,nitrogen,water vapour,and other constituents) in a room of capacity $25.0 \; m^{3}$ at a temperature of $27^{\circ} C$ and $1 \; atm$ pressure.

$A$ gas has a volume of $251 \,cm^3$ at $20^{\circ} C$ and a pressure of $78 \,cm$ of $Hg$. Find its volume at $NTP$. (in $\,cm^3$)

In the given $(V - T)$ diagram,what is the relation between pressures $P_1$ and $P_2 \,?$

$A$ gas at $27^{\circ}C$ has a volume $V$ and pressure $P$. On heating,its pressure is doubled and volume becomes three times. The resulting temperature of the gas will be ...... $^{\circ}C$.

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