Calculate the volume of gas at $1.25 \ atm$,if the volume occupied by the gas at $1 \ atm$ and at the same temperature is $25 \ mL$. (in $mL$)

If $P$,$V$,$M$,$T$ and $R$ are pressure,volume,molar mass,temperature and gas constant respectively,then for an ideal gas,the density is given by

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 the surroundings. Calculate the number of moles of gas used.

What will be the volume in $L$ of $2.8 \ g$ of carbon monoxide at $27 \ ^oC$ temperature and $0.821 \ atm$ pressure? $(R = 0.0821 \ L \ atm \ mol^{-1} K^{-1})$

$A$ flask of $1 \ L$ capacity is heated from $25 \ ^oC$ to $35 \ ^oC$. What volume of air (in $mL$) will be expelled from the flask?

The volume of a given mass of a gas is directly proportional to its Kelvin temperature at constant pressure. The above statement is known as . . . . . .