(B) According to the ideal gas law,$\frac{p_{1} V_{1}}{T_{1}} = \frac{p_{2} V_{2}}{T_{2}}$.Given: $T_{2} = 2 T_{1}$ and $p_{2} = \frac{p_{1}}{2}$.Subs

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will be $4$ times the original volume

(B) According to the ideal gas law,$\frac{p_{1} V_{1}}{T_{1}} = \frac{p_{2} V_{2}}{T_{2}}$.Given: $T_{2} = 2 T_{1}$ and $p_{2} = \frac{p_{1}}{2}$.Substituting these values into the equation:$\frac{p_{1} V_{1}}{T_{1}} = \frac{(p_{1} / 2) \times V_{2}}{2 T_{1}}$.Canceling $p_{1}$ and $T_{1}$ from both sides:$V_{1} = \frac{V_{2}}{4}$.Therefore,$V_{2} = 4 V_{1}$.The volume becomes $4$ times the original volume.

Class 11 Chemistry States of Matter Ideal gas equation and Related gas laws

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When the absolute temperature of an ideal gas is doubled and the pressure is halved,the volume of the gas

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A
will be half of the original volume
B
will be $4$ times the original volume
C
will be $2$ times the original volume
D
will be $1/4$ th of the original volume

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Ideal gas equation and Related gas laws

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At $25^{\circ} C$ and $760 \,mm \,Hg$ pressure,a gas occupies $600 \,mL$ volume. What will be its pressure at a height where the temperature is $10^{\circ} C$ and the volume of the gas is $640 \,mL$?

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At $25 \, ^\circ C$,a $3.7 \, g$ gas occupies the same volume as $0.184 \, g$ of $H_2$ gas at $17 \, ^\circ C$ under the same pressure. What is the molar mass of the gas?

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When the absolute temperature of an ideal gas is doubled and the pressure is halved,the volume of the gas

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At $25^{\circ} C$ and $760 \,mm \,Hg$ pressure,a gas occupies $600 \,mL$ volume. What will be its pressure at a height where the temperature is $10^{\circ} C$ and the volume of the gas is $640 \,mL$?

In terms of Charles' law,explain why $-273.15 \,^{\circ}C$ is the lowest possible temperature.

$A$ gas has a volume of $3.4 \ L$ at $25^{\circ} C$. What is the final temperature if the volume increases to $10.2 \ L$ at constant pressure (in $K$)?

$A$ mass of gas occupies $11.2 \ dm^3$ at $105 \ kPa$. What is its volume if the pressure is increased to $210 \ kPa$ at constant temperature (in $dm^3$)?

At $25 \, ^\circ C$,a $3.7 \, g$ gas occupies the same volume as $0.184 \, g$ of $H_2$ gas at $17 \, ^\circ C$ under the same pressure. What is the molar mass of the gas?

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