At 21°C,a gas cylinder containing nitrogen has an internal volume and pressure of 46.6 L and 1.50 × 10² atm.What mass of nitrogen gas is contained in the cylinder?

Question

Quizplus · Accepted Answer

We can use the ideal gas law to solve for the mass of nitrogen gas.

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

Rearranging the equation to solve for n:

n = PV/RT

Substituting the given values:

n = (1.50 × 10^(12) Pa)(46.6 L)/(8.314 J/mol K)(294 K)

n = 5.43 mol

To convert from moles to grams, we need to use the molar mass of nitrogen gas:

M(N2) = 28.02 g/mol

Multiplying the number of moles by the molar mass:

m = nM(N2)

m = (5.43 mol)(28.02 g/mol)

m = 152 g

Therefore, the mass of nitrogen gas in the cylinder is 8.11 × 10^(13) g, which corresponds to choice C.

At 21°C,a Gas Cylinder Containing Nitrogen Has an Internal Volume