Answer:
Partial pressure of H₂ = 499 mmHg
Partial pressure of Ar = 481 mmHg
Explanation:
We'll begin by calculating the number of mole of each gas. This can be obtained as follow:
For Hydrogen:
Molar mass of H₂ = 2 × 1 = 2 g/mol
Mass of H₂ = 0.291 g
Mole of H₂ =?
Mole = mass /molar mass
Mole of H₂ = 0.291/ 2
Mole of H₂ = 0.1455 mole
For Argon:
Molar mass of Ar = 40 g/mol
Mass of Ar = 5.62 g
Mole of Ar =?
Mole = mass /molar mass
Mole of Ar = 5.62 / 40
Mole of Ar = 0.1405 mole
Next, we shall determine the mole fraction of each gas. This can be obtained as follow:
Mole of H₂ = 0.1455 mole
Mole of Ar = 0.1405 mole
Total mole = 0.1455 + 0.1405
Total mole = 0.286 mole
Mole fraction of H₂ (nₕ₂) = mole of H₂ / total mole
Mole fraction of H₂ (nₕ₂) = 0.1455/0.286
Mole fraction of H₂ (nₕ₂) = 0.509
Mole fraction of Ar (nₐᵣ) = mole of Ar / total mole
Mole fraction of Ar (nₐᵣ) = 0.1405/0.286
Mole fraction of Ar (nₐᵣ) = 0.491
Finally, we shall determine the partial pressure of each gas. This can be obtained as follow:
For Hydrogen:
Mole fraction of H₂ (nₕ₂) = 0.509
Total pressure (Pₜ) = 980 mmHg
Partial pressure of H₂ (Pₕ₂) =?
Pₕ₂ = nₕ₂ × Pₜ
Pₕ₂ = 0.509 × 980
Partial pressure of H₂ (Pₕ₂) = 499 mmHg
For Argon:
Partial pressure of H₂ (Pₕ₂) = 499 mmHg
Total pressure (Pₜ) = 980 mmHg
Partial pressure of Ar (Pₐᵣ) =?
Pₜ = Pₕ₂ + Pₐᵣ
980 = 499 + Pₐᵣ
Collect like terms
980 – 499 = Pₐᵣ
481 = Pₐᵣ
Partial pressure of Ar (Pₐᵣ) = 481 mmHg
SUMMARY:
Partial pressure of H₂ (Pₕ₂) = 499 mmHg
Partial pressure of Ar (Pₐᵣ) = 481 mmHg
