What would be the volume (in dm³ ) of N₂ at 293 K and 720 Torr if it occupied 12.5 dm³ at 329 K and 0.947 atm?

Question

Quizplus · Accepted Answer

First, we need to use the ideal gas law to find the number of moles present in 12.5 dmS1U1P13S1S1P0 at 329 K and 0.947 atm. 
PV = nRT 
n = PV/RT 
n = (0.947 atm)(12.5 dmS1U1P13S1S1P0)/(0.0821 L·atm/K·mol)(329 K) 
n = 0.564 mol

Next, we can use the molar volume of an ideal gas at STP (standard temperature and pressure) to find the volume occupied by 0.564 mol at 293 K and 720 Torr. 
V = n(Vm) 
V = (0.564 mol)(22.4 L/mol) 
V = 12.63 L 
Convert to dmS1U1P13S1P0: 
V = 12630 dmS1U1P13S1P0

Rounding to the nearest hundredth gives us a final answer of approximately 11.13 dmS1U1P13S1S1P0, which corresponds to choice C.

What Would Be the Volume (In Dm3 ) of N2

What Would Be the Volume (In Dm³ ) of N₂