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?

1.62 L.

Explanation:

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.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

elements make up everything, and they combine to make compounds.

the answer is c