(B) Since the temperature is constant,we use Boyle's Law: $P_1 V_1 = P_2 V_2$.Given: $P_1 = 2 \, atm$,$V_1 = 500 \, cc$,$V_2 = 400 \, cc$.Substituting

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(B) Since the temperature is constant,we use Boyle's Law: $P_1 V_1 = P_2 V_2$.Given: $P_1 = 2 \, atm$,$V_1 = 500 \, cc$,$V_2 = 400 \, cc$.Substituting the values into the equation:$P_2 = P_1 \times \frac{V_1}{V_2}$$P_2 = 2 \times \frac{500}{400}$$P_2 = 2 \times 1.25 = 2.5 \, atm$.

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

Easy

$A$ sample of oxygen gas is compressed from a volume of $500 \, cc$ to $400 \, cc$ at a pressure of $2 \, atm$. If the temperature is kept constant,what pressure in $atm$ is required?

A
$1.2$
B
$2.5$
C
$4.7$
D
$5.0$

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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

The pressure of a given mass of gas at $20^{\circ}C$ is $P$. At constant volume,at what temperature in $^{\circ}C$ will the pressure of the gas become $2P$?

Easy

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The pressure $Vs$ temperature graph of an ideal gas is shown in the figure. If the density of the gas at point $A$ is $\rho _0$,what will be the density at point $B$?

Medium

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An ideal gas is expanding such that $PT^2 = \text{constant}$. The coefficient of volume expansion of the gas is

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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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The lowest pressure (the best vacuum) that can be created in the laboratory at $27^{\circ}C$ is $10^{-11} \; mm$ of $Hg$. At this pressure,the number of ideal gas molecules per $cm^{3}$ will be:

Medium

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$A$ sample of oxygen gas is compressed from a volume of $500 \, cc$ to $400 \, cc$ at a pressure of $2 \, atm$. If the temperature is kept constant,what pressure in $atm$ is required?

Similar Questions

The pressure of a given mass of gas at $20^{\circ}C$ is $P$. At constant volume,at what temperature in $^{\circ}C$ will the pressure of the gas become $2P$?

The pressure $Vs$ temperature graph of an ideal gas is shown in the figure. If the density of the gas at point $A$ is $\rho _0$,what will be the density at point $B$?

An ideal gas is expanding such that $PT^2 = \text{constant}$. The coefficient of volume expansion of the gas is

$A$ 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 ...... $^{\circ}C$.

The lowest pressure (the best vacuum) that can be created in the laboratory at $27^{\circ}C$ is $10^{-11} \; mm$ of $Hg$. At this pressure,the number of ideal gas molecules per $cm^{3}$ will be:

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