(C) We know the ideal gas equation is $PM = dRT$,where $P$ is pressure,$M$ is molar mass,$d$ is density,$R$ is the gas constant,and $T$ is temperature

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(C) We know the ideal gas equation is $PM = dRT$,where $P$ is pressure,$M$ is molar mass,$d$ is density,$R$ is the gas constant,and $T$ is temperature.At constant pressure and for a given gas,$d \times T = \text{constant}$.Therefore,$d_1 T_1 = d_2 T_2$.Given: $d_1 = d$,$T_1 = 27\,^oC = (273 + 27)\,K = 300\,K$,and $d_2 = 0.75\,d$.Substituting the values: $d \times 300 = 0.75\,d \times T_2$.$T_2 = \frac{300}{0.75} = 400\,K$.

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

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At a temperature of $27\,^oC$ and a pressure of $1\,atm$,the density of a gas is $d$. At constant pressure,at what temperature will its density become $0.75\,d$?

A
$20\,^oC$
B
$30\,^oC$
C
$400\,K$
D
$300\,K$

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At a temperature of $27\,^oC$ and a pressure of $1\,atm$,the density of a gas is $d$. At constant pressure,at what temperature will its density become $0.75\,d$?

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