Another type of Ideal Gas Law problem is where they change two or more variables keeping the others fixed. For example, consider a sample of gas kept at constant temperature (so its amount is fixed, too). If the gas is initially at 593.9mmHg and 0.864 Liters, then what will be the final volume if the pressure in the container was raised to 988mmHg ? (3 sig figs) QUESTION 2 Since n equals moles and since moles =g/MM (grams divided by Molar Mass), then one can plug in (g/MM) for n in PV=nRT. That gives PV=(g/MM)RT whcih rearranges to (MM)PV=gRT. If we divide both sides by V, we get (MM)P=( g/R)RT.... g/V is grams per Liter which is density So an alternative form of the Ideal Gas Law equation is (MM)P-dRT where MM is Molar Mass, P is still Pressure, T and R are still the same and d is density of the gas. So, determine the density of CH4(g) at 832mmHg and 44C. Three sig figs