If $20 \ cm^3$ of gas at $1 \ atm$ is expanded to $50 \ cm^3$ at constant $T$,what is the final pressure?

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 $2 \, \text{moles}$ of an ideal gas occupy a volume of $44.8 \, L$ at a temperature of $546 \, K$,what will be the pressure in $atm$?

For a fixed amount of gas at constant pressure,provide the plot of volume $(V)$ versus temperature $(T)$ in Kelvin. What does it represent?

For one mole of an ideal gas, the slope of $V$ vs. $T$ curve at a constant pressure of $2 \ atm$ is $X \ L \ mol^{-1} \ K^{-1}$. The value of the ideal universal gas constant '$R$' in terms of $X$ is

At a given temperature,the density of an ideal gas is proportional to $(P = \text{pressure of ideal gas})$