The temperature of $4.0 \ mol$ of a gas occupying $5 \ dm^3$ at $3.32 \ bar$ is $(R = 0.083 \ bar \ dm^3 \ K^{-1} \ mol^{-1})$. (in $K$)

The volume occupied by $4.75 \, g$ of acetylene gas at $50^{\circ} C$ and $740 \, mm \, Hg$ pressure is ....... $L$.
(Rounded off to the nearest integer)
$[$ Given $R = 0.0826 \, L \, atm \, K^{-1} \, mol^{-1} ]$

For an ideal gas obeying Boyle's Law,which of the following is correct? ($K$ is a constant)

Explain: Gay-Lussac's Law.

When the absolute temperature of an ideal gas is doubled and the pressure is halved,the volume of the gas

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