The density of ammonia gas at $27^{\circ}C$ and $3 \, atm$ pressure is approximately:

At constant pressure,the temperature of $20 \ L$ of helium gas is increased from $100 \ K$ to $300 \ K$. What will be the change in volume in $L$?

$A$ and $B$ are ideal gases. At $T(K)$,$2 \ L$ of $A$ with a pressure of $1 \ bar$ is mixed with $4 \ L$ of $B$ with a pressure $p_B \ bar$ in a $100 \ L$ flask. The pressure exerted by the gaseous mixture is $0.1 \ bar$. What is the value of $p_B$ in $bar$?

The density of an ideal gas can be given by where $P$,$V$,$M$,$T$ and $R$ respectively denote pressure,volume,molar mass,temperature and universal gas constant.

The value of the gas constant $R$ depends on which of the following?

In terms of Charles' law,explain why $-273^{\circ} C$ is the lowest possible temperature.