(C) From the ideal gas equation,$PV = nRT$,we have $T = (P/nR)V$. For a fixed amount of gas ($n$ is constant),the slope of the $T-V$ graph is given by

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(C) From the ideal gas equation,$PV = nRT$,we have $T = (P/nR)V$. For a fixed amount of gas ($n$ is constant),the slope of the $T-V$ graph is given by $m = P/nR$. Since $n$ and $R$ are constants,the slope $m$ is directly proportional to the pressure $P$. Therefore,a steeper slope in the $T-V$ graph corresponds to a higher pressure. Looking at the graph,the slope of the curve for $P_1$ is the steepest,followed by $P_2$,and then $P_3$. Thus,the correct relation is $P_1 > P_2 > P_3$.

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

The following graph represents the $T-V$ curves of an ideal gas (where $T$ is the temperature and $V$ is the volume) at three pressures $P_1, P_2$ and $P_3$ compared with those of Charles's law represented as dotted lines. Then the correct relation is:

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A
$P_1 > P_3 > P_2$
B
$P_2 > P_1 > P_3$
C
$P_1 > P_2 > P_3$
D
$P_3 > P_2 > P_1$

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Class 11

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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

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The figure shows the volume $V$ versus temperature $T$ graphs for a certain mass of a perfect gas at two constant pressures of $P_1$ and $P_2$. What inference can you draw from the graphs?

MediumAIIMS 2014

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When the temperature of a gas in a closed vessel is increased by $2.4^{\circ} C$, its pressure increases by $0.5 \%$. The initial temperature of the gas is (in $^{\circ} C$)

MediumTS EAMCET 2025

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If the pressure of a gas contained in a closed vessel is increased by $0.4\%$ when heated by $1\,^{\circ}C$,the initial temperature must be

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The pressure $P$,volume $V$,and temperature $T$ of a gas in jar $A$ are given. Another gas in jar $B$ has pressure $2P$,volume $V/4$,and temperature $2T$. The ratio of the number of molecules in jar $A$ to jar $B$ is:

MediumAIIMS 1982

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The following graph represents the $T-V$ curves of an ideal gas (where $T$ is the temperature and $V$ is the volume) at three pressures $P_1, P_2$ and $P_3$ compared with those of Charles's law represented as dotted lines. Then the correct relation is:

Similar Questions

The figure shows the volume $V$ versus temperature $T$ graphs for a certain mass of a perfect gas at two constant pressures of $P_1$ and $P_2$. What inference can you draw from the graphs?

An electron tube was sealed off during manufacture at a pressure of $1.2 \times 10^{-7} \text{ mm}$ of mercury at $27^{\circ}C$. Its volume is $100 \text{ cm}^3$. The number of molecules that remain in the tube is

When the temperature of a gas in a closed vessel is increased by $2.4^{\circ} C$, its pressure increases by $0.5 \%$. The initial temperature of the gas is (in $^{\circ} C$)

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The pressure $P$,volume $V$,and temperature $T$ of a gas in jar $A$ are given. Another gas in jar $B$ has pressure $2P$,volume $V/4$,and temperature $2T$. The ratio of the number of molecules in jar $A$ to jar $B$ is:

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