(A) From the ideal gas equation,$PV = nRT = (m/M)RT$.Since density $d = m/V$,we have $PM = dRT$,which implies $d = PM / RT$.Therefore,$d \propto P / T

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$d_2 = d_1 [T_1 P_2 / T_2 P_1]$

(A) From the ideal gas equation,$PV = nRT = (m/M)RT$.Since density $d = m/V$,we have $PM = dRT$,which implies $d = PM / RT$.Therefore,$d \propto P / T$.This gives the relation $\frac{d_2}{d_1} = \frac{P_2 / T_2}{P_1 / T_1} = \frac{P_2 T_1}{P_1 T_2}$.Thus,$d_2 = d_1 [T_1 P_2 / T_2 P_1]$.

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

Medium

Which relation represents the change in density of an ideal gas with changes in temperature and pressure?

A
$d_2 = d_1 [T_1 P_2 / T_2 P_1]$
B
$d_2 = d_1 [T_1 T_2 / P_1 P_2]$
C
$d_2 = d_1 [T_1 P_1 / T_2 P_2]$
D
$d_2 = d_1 [T_2 P_2 / T_1 P_1]$

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States of Matter

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Ideal gas equation and Related gas laws

At $27\, ^\circ C$ temperature and $1\, bar$ pressure,the volume of a gas is $25\, L$. If the temperature becomes $77\, ^\circ C$ at constant pressure,calculate the volume of the gas. (in $, L$)

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Densities of a gas at different conditions are in the ratio $1:2$ and their temperatures are in the ratio $2:1$,then the ratio of their respective pressure is :-

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What is the weight of $CH_4$ gas in a $9 \ L$ cylinder at $27 \ ^oC$ temperature and $1 \ atm$ pressure in $g$?

Medium

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When the applied pressure is $16 \ atm$,the temperature is $27 \ ^oC$,and the volume is $9 \ L$,what will be the weight of $CH_4$ gas in $gm$? (Given $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$)

Easy

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Calculate the new volume of a gas at constant pressure when temperature is increased to $546 \ K$.
[Initial volume of a gas at $273 \ K$ is $4 \ dm^3$] (in $dm^3$)

MediumMHT CET 2022

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Which relation represents the change in density of an ideal gas with changes in temperature and pressure?

Similar Questions

At $27\, ^\circ C$ temperature and $1\, bar$ pressure,the volume of a gas is $25\, L$. If the temperature becomes $77\, ^\circ C$ at constant pressure,calculate the volume of the gas. (in $, L$)

Densities of a gas at different conditions are in the ratio $1:2$ and their temperatures are in the ratio $2:1$,then the ratio of their respective pressure is :-

What is the weight of $CH_4$ gas in a $9 \ L$ cylinder at $27 \ ^oC$ temperature and $1 \ atm$ pressure in $g$?

When the applied pressure is $16 \ atm$,the temperature is $27 \ ^oC$,and the volume is $9 \ L$,what will be the weight of $CH_4$ gas in $gm$? (Given $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$)

Calculate the new volume of a gas at constant pressure when temperature is increased to $546 \ K$. [Initial volume of a gas at $273 \ K$ is $4 \ dm^3$] (in $dm^3$)

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Calculate the new volume of a gas at constant pressure when temperature is increased to $546 \ K$.
[Initial volume of a gas at $273 \ K$ is $4 \ dm^3$] (in $dm^3$)