If a 4.00 L container is filled with N₂ to a pressure of 895 torr at 53.0°C, calculate the mass of the nitrogen in the container. A)0.176 g B)4.93 g C)134 g D)5.68 g E)0.202 g

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of nitrogen gas in the container using the Ideal Gas Law:
PV = nRT
where P is the pressure in atm, V is the volume in liters, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
Converting the given pressure to atm and the temperature to Kelvin, we get:
(895 torr) / (760 torr/atm) = 1.18 atm
53.0°C + 273.15 = 326.15 K
Substituting these values and solving for n, we get:
n = (1.18 atm * 4.00 L) / (0.08206 L atm/mol K * 326.15 K) = 0.172 mol
Next, we can use the molar mass of nitrogen gas (28.0134 g/mol) to calculate the mass of nitrogen in the container:
mass = n * molar mass = 0.172 mol * 28.0134 g/mol = 4.93 g
Therefore, the answer is B.

If a 400 L Container Is Filled with N2 to a Pressure

If a 400 L Container Is Filled with N₂ to a Pressure