Question

A mixture of gases contains 12.47 g of H₂, 1.98 g of O₂, and 8.15 g of N₂. If the total pressure of the mixture is 2.35 atm, what is the partial pressure of each component?

a) H₂ = 0.56 atm, O₂ = 0.09 atm, N₂ = 1.70 atm

b) H₂ = 1.20 atm, O₂ = 0.18 atm, N₂ = 0.97 atm

c) H₂ = 0.85 atm, O₂ = 0.14 atm, N₂ = 0.36 atm

d) H₂ = 2.12 atm, O₂ = 0.33 atm, N₂ = 0.50 atm

Answer 1

To calculate the partial pressure of each component, you need to calculate the moles of each gas using their respective molar masses, then calculate the mole fraction of each component, and finally use Dalton's law of partial pressure to calculate the partial pressure of each component.

Step-by-step explanation:

To calculate the partial pressure of each component, we first need to calculate the moles of each gas using their respective molar masses. The molar mass of H₂ is 2 g/mol, O₂ is 32 g/mol, and N₂ is 28 g/mol.

The moles of H₂ = 12.47 g / 2 g/mol = 6.235 mol

The moles of O₂ = 1.98 g / 32 g/mol = 0.061875 mol

The moles of N₂ = 8.15 g / 28 g/mol = 0.290179 mol

Next, we will calculate the mole fraction of each component.

The mole fraction of H₂ = moles of H₂ / total moles = 6.235 mol / (6.235 mol + 0.061875 mol + 0.290179 mol) = 0.944

The mole fraction of O₂ = 0.059

The mole fraction of N₂ = 0.28

Finally, we can calculate the partial pressure of each component using Dalton's law of partial pressure.

The partial pressure of H₂ = mole fraction of H₂ * total pressure = 0.944 * 2.35 atm = 2.2184 atm

The partial pressure of O₂ = 0.059 * 2.35 atm = 0.13865 atm

The partial pressure of N₂ = 0.28 * 2.35 atm = 0.658 atm