A balloon contains 3.9 moles of helium at a pressure of 234 kPa and 67°C temperature. What is the balloon's volume in liters?

47.1 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 = 234.0 kPa/101.325 ≅ 2.31 atm).

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

n is the no. of moles of the gas in mol (n = 3.9 mol).

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

T is the temperature of the gas in K (T = 67.0 °C + 273.15 = 340.15 K).

The volume of the gas = nRT/P.

∴ V = nRT/P = (3.9 mol) (0.082 L. atm/mol. K) (340.15 K) / (2.31 atm) = 47.1 L.