At $273 \, K$ temperature and $1 \, bar$ pressure,if the volume of a gas increases by $20 \%$,what temperature is required assuming pressure remains constant (in $, K$)?

At $27\, ^\circ C$ temperature and $1\, bar$ pressure,the volume of a gas is $25\, L$. If the temperature becomes $77\, ^\circ C$ at constant pressure,calculate the volume of the gas. (in $, L$)

The graph of pressure $(P)$ versus density $(d)$ is shown for an ideal gas at two temperatures $T_1$ and $T_2$. Which of the following is correct?

If the density of a gas at sea level is $1.5 \ mg \ L^{-1}$,find the density of that gas on Mount Abu,where the pressure is $0.5 \ bar$. (Assume pressure at sea level is $1.0 \ bar$ and use the formula $\frac{d_1}{d_2} = \frac{p_1}{p_2}$) (in $mg \ L^{-1}$)

If two moles of an ideal gas at $546 \ K$ occupy a volume of $44.8 \ L$,what is the pressure of the ideal gas at $546 \ K$ (in $atm$)? $(R = 0.0821 \ L \ atm \ mol^{-1} \ K^{-1})$

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