Question

You have a fixed container with a volume of 5.00 L that contains 35.0 g nitrogen gas (N2). If the temperature is 298 K, calculate the pressure in the container. (R = 0.0821 L∙atm/mol∙K)

a) 171 atm
b) 6.12 atm
c) 30.6 atm
d) 856 atm

Answer 1

To find the pressure of nitrogen gas in the container, the ideal gas law is used; after calculating the moles of nitrogen using its molar mass, the result indicates a pressure of approximately 6.12 atm.

Step-by-step explanation:

To calculate the pressure in the container, one can use the ideal gas law, given by PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvins.

Firstly, we need to calculate the number of moles (n) of nitrogen gas (N₂). The molar mass of N₂ is 28.01 g/mol, therefore:

n = mass / molar mass = 35.0 g / 28.01 g/mol ≈ 1.249 moles

Next, using the ideal gas law and given the constants:

PV = nRT
⇒ P = (nRT) / V
⇒ P = (1.249 moles) * (0.0821 L⋅atm/mol⋅K) * (298 K) / (5.00 L)
⇒ P ≈ 6.12 atm

Therefore, the pressure in the container is approximately 6.12 atm.