What is the density of N2O at 750 torr and 30•C?

Mass = 14 * 2 + 16 = 44 grams

The volume of one mole of a gas at standard temperature and pressure is 22.4 liters. Let’s use the following equation to determine the volume of mole of this gas at a pressure of 750 torr and a temperature of 30˚C.

P1 * V1 ÷ T1 = P2 * V2 ÷ T2

T1 = 30 + 273 = 303
P2 = 760 torr
T2 = 273

750 * V1 ÷ 303 = 760 * 22.4 ÷ 273

V1 * 204,750 = 515,827.2
V = 515,827.2 ÷ 204,750

The volume is approximately 25 liters.

Density = 44 ÷ (515,827.2 ÷ 204,750)

This is approximately 1.75 g/L. I hope this is helpful for you.

n / V = P / RT = (750 torr) / ((62.36367 L torr/K mol) x (30 + 273) K) = 0.03969054 mol/L

(44.0128 g N2O/mol) x (0.03969054 mol/L) = 1.75 g/L