Since the gas it is getting compressed with a change on temperature, we consider that the pressure is constant, and of course the number of mole is constant (same gas), therefore, from the $PV=nRT$ we can say:
And this is old $"Charles' Law..."$ Now $"STP"$ specifies (depending on your syllabus) $298*K$ and (near to) $1*atm$... Given $VpropT$, $V=kT$...solving for $k$, $k=V/T$...but this should apply at all temperatures...
And $1*atm-=760*mm*Hg$ or rather $1*atm$ will support a column of mercury that is $760* mm$ high...and I truly hope you have seen such a column because the health and safety...
You'd use , which links an ideal gas' volume to its temperature if pressure and number of moles are kept constant. The mathematical formula is this $V_1/T_1 = V_2/T_2$...
The idea here is that the volume and the temperature of a gas have a direct relationship when the pressure and the number of moles of gas are being kept...