When the temperature of a flask with a capacity of $1 \ L$ is increased from $25 \ ^oC$ to $35 \ ^oC$,calculate the volume of air in $mL$ that escapes from the flask.

Two separate identical containers contain Gas $A$ $(Mw = 40 \ g \ mol^{-1})$ and gas $B$ $(Mw = x \ g \ mol^{-1})$ in the mass ratio $5 : 8$ under similar conditions of temperature and pressure. The value of $x$ is $:-$

An ideal gas expands isothermally and reversibly from $10 \ m^{3}$ to $20 \ m^{3}$ at $300 \ K$ performing $5.187 \ kJ$ of work on surroundings. Calculate the number of moles of gas undergoing expansion? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

On what factors do the values of the gas constant $R$ depend? What is its unit?

If a gas expands from $20 \ cm^3$ to $50 \ cm^3$ at a constant temperature $(T)$ under a pressure of $1 \ atm$,what will be the final pressure?

At $127 \, ^oC$ temperature,the volume of a gas is $3 \, L$. If the volume of the gas becomes half at constant pressure,calculate the final temperature in Kelvin. (in $, K$)