Question

A sample of 56 grams of nitrogen (N2) gas at 760 torr and 0°C occupies a volume of ______ liters.

A. 11.2
B. 22.4
C. 44.8
D. 89.6

Answer 1

The volume of the nitrogen gas is approximately 22.4 liters. V = (56 g / 28.01 g/mol) * (0.0821 L.atm/mol.K) * (273 K) / 760 torr , V ≈ 22.4 L

Step-by-step explanation:

The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure.

To find the volume, we can use the ideal gas law equation:

V = (nRT) / P

Here, n is the number of moles of the gas, R is the ideal gas constant, T is the temperature in Kelvin, and P is the pressure in atmospheres.

In this case, we are given the mass of nitrogen gas (N2), which we can convert to moles using its molar mass, and the temperature and pressure.

Plugging in the values:

V = (56 g / 28.01 g/mol) * (0.0821 L.atm/mol.K) * (273 K) / 760 torr

V ≈ 22.4 L