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

The variation of volume of an ideal gas with its number of moles $(n)$ is obtained as a graph at $300 \ K$ and $1 \ atm$ pressure. What is the slope of the graph?

Define the gas constant $R$ in terms of work.

At constant pressure,the volume of a fixed mass of an ideal gas is directly proportional to

An ideal gas on isothermal reversible compression from $10 \ L$ to $5 \ L$ performs $1730 \ J$ of work at $300 \ K$. Calculate the number of moles of gas involved in the compression? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

When $2 \ g$ of a gaseous substance $A$ is introduced into an initially evacuated flask at $25^{\circ} C$,the pressure is found to be $1 \ atm$. $3 \ g$ of another gaseous substance $B$ is added to it at the same temperature and pressure. The final pressure is found to be $1.5 \ atm$. Assuming ideal gas behaviour,the ratio of molar masses of $A$ and $B$ is: