Match the following gas laws with their respective equations.

For $1 \ mol$ of an ideal gas at a constant temperature $T,$ the plot of $(\log \ P)$ against $(\log \ V)$ is a ($P :$ Pressure,$V:$ Volume)

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? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

If a gas occupies a volume of $1.5 \, L$ at a pressure of $75 \, cm \, Hg$,then at the same temperature,the volume of the gas at a pressure of $50 \, cm \, Hg$ will be ........... $L$. (in $.25$)

At $300 \ K$,the following graph is obtained for one mole of an ideal gas. If its pressure is $10 \ atm$,then its volume (in $L$) will be

At $0^{\circ} C$,a gas occupies $22.4 \ L$. What is the temperature in Kelvin required to reach a volume of $224 \ L$ (in $K$)?