Question

What are the partial pressures And the total pressures of the gases in a 3.7 L balloon, if the balloon is filled with 2.6 moles of gas 1, and 4.8 moles of gas 2 at 58 degrees Celsius?

Answer 1

number of moles of gas 1 = 2.6 moles

number of moles of gas 2 = 4.8 moles

Total number of moles = 2.6 + 4.8 = 7.4 moles

Temperature = 57°C = (273 + 58)K = 331K

mole fraction of gas 1 = $2.6/ 7.4 =0.351$

mole fraction of gas 2 = $4.8/7.4= 0.649$

Using, $PV =nRT$

$P = \dfrac{nRT}{V} = \dfrac{7.4× 8.314× 331}{3.7×10^{-3}}$

$= 5.504MPa$

Partial pressure of 1 $= 0.351× 5.5MPa$ $= 1.93MPa$

Partial pressure of 2 = $0.649 × 5.5MPa$

$= 3.57MPa$