(B) From the ideal gas equation, $PV = nRT$, where $n$ is the number of moles. The number of molecules $N$ is given by $N = nN_A$, where $N_A$ is Avog

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(B) From the ideal gas equation, $PV = nRT$, where $n$ is the number of moles. The number of molecules $N$ is given by $N = nN_A$, where $N_A$ is Avogadro's number.Thus, $N = \frac{PVN_A}{RT}$.For jar $A$: $N_A = \frac{PVN_A}{RT}$.For jar $B$: $N_B = \frac{(2P)(\frac{V}{4})N_A}{R(2T)} = \frac{\frac{PV}{2}N_A}{2RT} = \frac{PVN_A}{4RT}$.The ratio of the number of molecules in jar $B$ to jar $A$ is $\frac{N_B}{N_A} = \frac{\frac{PVN_A}{4RT}}{\frac{PVN_A}{RT}} = \frac{1}{4}$.Therefore, the ratio is $1 : 4$.

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

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Gas at pressure $P$, temperature $T$, and volume $V$ is filled in jar $A$. Another jar $B$ is filled with gas having parameters $2P, \frac{V}{4}, 2T$. The ratio of the number of molecules of jar $B$ to those of jar $A$ is:

MHT CET 2026 All MHT CET

A
$1 : 2$
B
$1 : 4$
C
$2 : 1$
D
$4 : 1$

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Class 11 Questions

Class 11

Physics Questions

Chapter

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

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$A$ gas of certain mass filled in a closed cylinder at a pressure of $3.23 \ kPa$ has a temperature of $50^{\circ} C$. The gas is now heated until its absolute temperature is doubled. The modified pressure is . . . . . . $Pa$.

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Gas at pressure $P$, temperature $T$, and volume $V$ is filled in jar $A$. Another jar $B$ is filled with gas having parameters $2P, \frac{V}{4}, 2T$. The ratio of the number of molecules of jar $B$ to those of jar $A$ is:

Similar Questions

What will be the volume occupied by $4.5 \, kg$ of water at $STP$ if the intermolecular forces are neglected?

$A$ balloon contains $500 \ m^3$ of helium at $27^{\circ}C$ and $1 \ atm$ pressure. The volume of the helium at $-3^{\circ}C$ temperature and $0.5 \ atm$ pressure will be ..... $m^3$.

What is Boltzmann's constant?

$A$ gas of certain mass filled in a closed cylinder at a pressure of $3.23 \ kPa$ has a temperature of $50^{\circ} C$. The gas is now heated until its absolute temperature is doubled. The modified pressure is . . . . . . $Pa$.

$A$ gas at $27^{\circ}C$ has a volume $V$ and pressure $P$. If it is heated such that the pressure becomes double and the volume becomes triple,what is the final temperature in $^{\circ}C$?

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