The total pressure of a gaseous mixture of 2.8g of n^2, 3.2 g of o^2 and o.5 g of h^2 is 4.5atm. calculate the partial pressure of h^2 gas
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- Total pressure = 4.5 atm
- Amount of gases present in mixture are 2.8g of N₂ , 3.2 g of O₂ and 0.5g of H₂
- Partial pressure of H₂ gas
Number of moles of a substance is given by ,
a] Given weight of N₂ = 2.8g
Atomic weight of N₂ = 28g
Number of moles of N₂ is ,
b] Given weight of O₂ = 3.2 g
Atomic weight of O₂ = 32g
c] Given weight of H₂ = 0.5 g
Atomic weight of H₂ = 2
Total number of moles in the given mixture = 0.1 + 0.1 + 0.25 = 0.45 mol
Mole fraction of the first gas in the mixture is given by,
Mole fraction of H₂ is ,
We have ,
- Mole fraction of H₂ = 0.5
- Total pressure in the mixture = 4.5 atm
Partial pressure of any gas in the mixture is given by,
Where ,
- p is partial pressure
- m is mole fraction of the certain gas
- P is total pressure in the mixture
Partial pressure of H₂ is ,
∴ The partial pressure of H₂ in the given mixture is 2.25 atm
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