(A) Given: Initial pressure $P_1 = 1 \,atm = 1.01 \times 10^5 \,N/m^2$. Initial volume $V_1 = 1 \,m^3$. Initial temperature $T_1 = 300 \,K$. Final vol

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(A) Given: Initial pressure $P_1 = 1 \,atm = 1.01 \times 10^5 \,N/m^2$. Initial volume $V_1 = 1 \,m^3$. Initial temperature $T_1 = 300 \,K$. Final volume $V_2 = 2V_1 = 2 \,m^3$. Final temperature $T_2 = 2T_1 = 600 \,K$. Using the ideal gas law equation $\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$: $P_2 = P_1 \times \frac{V_1}{V_2} \times \frac{T_2}{T_1}$ $P_2 = (1.01 \times 10^5) \times \frac{1}{2} \times \frac{600}{300}$ $P_2 = (1.01 \times 10^5) \times \frac{1}{2} \times 2$ $P_2 = 1.01 \times 10^5 \,N/m^2 \approx 10^5 \,N/m^2$.

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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An ideal gas at atmospheric pressure has a temperature of $300 \,K$ and a volume of $1 \,m^3$. If its temperature and volume are both doubled,its pressure will be ...........

A
$10^5 \,N/m^2$
B
$2 \times 10^5 \,N/m^2$
C
$0.5 \times 10^5 \,N/m^2$
D
$4 \times 10^5 \,N/m^2$

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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

We have a jar filled with gas characterized by parameters $P, V, T$ and another jar $B$ filled with gas having parameters $2P, V/4, 2T$,where symbols have their usual meaning. The ratio of the number of molecules in jar $A$ to those in jar $B$ is

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Why is an increase in the temperature of a gas at constant volume and constant pressure not possible?

Easy

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What is the number of oxygen molecules in a cylinder of volume $1 \ m^3$ at $27^{\circ}C$ and $13.8 \ Pa$? (Boltzmann constant $k = 1.38 \times 10^{-23} \ JK^{-1}$)

Easy

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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?

MediumIIT 1982

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Equal masses of $N_2$ and $O_2$ gases are filled in containers $A$ and $B$ respectively. The volume of container $B$ is twice the volume of container $A$. What is the ratio of the pressure in container $A$ to that in container $B$?

Medium

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An ideal gas at atmospheric pressure has a temperature of $300 \,K$ and a volume of $1 \,m^3$. If its temperature and volume are both doubled,its pressure will be ...........

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We have a jar filled with gas characterized by parameters $P, V, T$ and another jar $B$ filled with gas having parameters $2P, V/4, 2T$,where symbols have their usual meaning. The ratio of the number of molecules in jar $A$ to those in jar $B$ is

Why is an increase in the temperature of a gas at constant volume and constant pressure not possible?

What is the number of oxygen molecules in a cylinder of volume $1 \ m^3$ at $27^{\circ}C$ and $13.8 \ Pa$? (Boltzmann constant $k = 1.38 \times 10^{-23} \ JK^{-1}$)

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?

Equal masses of $N_2$ and $O_2$ gases are filled in containers $A$ and $B$ respectively. The volume of container $B$ is twice the volume of container $A$. What is the ratio of the pressure in container $A$ to that in container $B$?

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