Question

a 2 ltr flask contains 1.6 g of CH4 and 0.5 g of hydrogen at 27°C .calculate the partial pressure of each gas in the mixture and hence calculate the total pressure

Answer 1

No. of moles of
CH4 = 1.6/16 = 0.1 mole
H2 = 0.5/2 = 0.25 mole
Total moles = n = 0.1 + 0.25 = 0.35

PV = nRT
P = nRT / V
P = (0.35 × 0.0821 × 300) / 2
P = 4.31 atm
Total pressure of mixture = 4.31 atm

Partial pressure of CH4
p = (No. of moles of CH4 / Total moles) × Pressure of mixture
= (0.1 / 0.35) × 4.31
= 1.23 atm

Partial pressure of H2
p = (No. of moles of H2 / Total moles) × Pressure of mixture
= (0.25 / 0.35) × 4.31
= 3.0 atm

Answer 2

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