(C) Using the ideal gas equation: $PV = \frac{m}{M}RT$,where $P$ is pressure,$V$ is volume,$m$ is mass,$M$ is molar mass,$R$ is the universal gas cons

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(C) Using the ideal gas equation: $PV = \frac{m}{M}RT$,where $P$ is pressure,$V$ is volume,$m$ is mass,$M$ is molar mass,$R$ is the universal gas constant,and $T$ is temperature.Since $P$,$V$,$m$,and $R$ are the same for both gases,we have $T = \frac{PVM}{mR}$.This implies $T \propto M$.The molar mass of helium $(M_{He} = 4 \ g/mol)$ is less than the molar mass of nitrogen $(M_{N_2} = 28 \ g/mol)$.Therefore,$T_{helium} < T_{nitrogen}$.

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

Medium

You have two containers of equal volume. One is full of helium gas. The other holds an equal mass of nitrogen gas. Both gases have the same pressure. How does the temperature of the helium compare to the temperature of the nitrogen?

A
$T_{helium} > T_{nitrogen}$
B
$T_{helium} = T_{nitrogen}$
C
$T_{helium} < T_{nitrogen}$
D
can't be said

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Kinetic Theory

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

$A$ container $X$ has a volume double that of container $Y$,and both are connected by a thin tube. Both contain the same ideal gas. The temperature of $X$ is $200\,K$ and that of $Y$ is $400\,K$. If the mass of the gas in $X$ is $m$,then the mass of the gas in $Y$ will be:

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$A$ pressure cooker contains air at $1$ atm and $30^\circ C$. If the safety valve of the cooker blows when the inside pressure $\ge 3$ atm,then the maximum temperature of the air inside the cooker can be .... $^\circ C$.

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The number of molecules in $1 \, cm^{3}$ of an ideal gas at $N.T.P.$ is:

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The equation of state for $5 \, g$ of oxygen at a pressure $P$ and temperature $T$,when occupying a volume $V$,will be (where $R$ is the gas constant).

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Which one of the following graphs represents the behavior of an ideal gas at a constant temperature?

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You have two containers of equal volume. One is full of helium gas. The other holds an equal mass of nitrogen gas. Both gases have the same pressure. How does the temperature of the helium compare to the temperature of the nitrogen?

Similar Questions

$A$ container $X$ has a volume double that of container $Y$,and both are connected by a thin tube. Both contain the same ideal gas. The temperature of $X$ is $200\,K$ and that of $Y$ is $400\,K$. If the mass of the gas in $X$ is $m$,then the mass of the gas in $Y$ will be:

$A$ pressure cooker contains air at $1$ atm and $30^\circ C$. If the safety valve of the cooker blows when the inside pressure $\ge 3$ atm,then the maximum temperature of the air inside the cooker can be .... $^\circ C$.

The number of molecules in $1 \, cm^{3}$ of an ideal gas at $N.T.P.$ is:

The equation of state for $5 \, g$ of oxygen at a pressure $P$ and temperature $T$,when occupying a volume $V$,will be (where $R$ is the gas constant).

Which one of the following graphs represents the behavior of an ideal gas at a constant temperature?

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