An airbag generates 1.8g of nitrogen gas (N2, molar mass = 28.0 g/mol) at a pressure of 101.3 kPa and a temperature of 34°C. What volume, in liters, will it occupy?

Question

Chemistry

Brynlee Booth

1 December, 13:07

An airbag generates 1.8g of nitrogen gas (N2, molar mass = 28.0 g/mol) at a pressure of 101.3 kPa and a temperature of 34°C. What volume, in liters, will it occupy?

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Answers (1)

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Darion Barker · Answer 1

1.62 L.

Explanation:

To solve these problems, we can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm (P = 101.3 kPa/101.325 ≅ 1.0 atm).

V is the volume of the gas in L (V = ? L).

n is the no. of moles of the gas in mol.

R is the general gas constant (R = 0.082 L. atm/mol. K),

T is the temperature of the gas in K (T = 34.0 °C + 273.15 = 307.15 K).

The volume of the gas = nRT/P.

P = 1.0 atm, V = ? L, R = 0.082 L. atm/mol. K, n = mass/molar mass = (1.8 g) / (28.0 g/mol) = 0.0642 mol.

∴ V = nRT/P = (0.0642 mol) (0.082 L. atm/mol. K) (307.15 K) / (1.0 atm) = 1.62 L.