What is the pressure of 800 .G of nitrogen gas at 25.00°C at a volume of 5.0 L?

Question

Quizplus · Accepted Answer

Using the ideal gas law, PV = nRT, we can calculate the pressure:
P = nRT/V
n = 800 g / 28 g/mol = 28.57 mol
R = 0.082 L atm/mol K
T = 25.00°C + 273.15 = 298.15 K
V = 5.0 L
P = (28.57 mol)(0.082 L atm/mol K)(298.15 K) / 5.0 L = 139.9 atm
Converting to Torr (1 atm = 760 Torr), we get:
P = 139.9 atm x 760 Torr/atm = 106,384 Torr
Rounding to 3 significant figures, the answer is D) 140 Torr.

What Is the Pressure of 800