Final answer:
The partial pressure of N₂ in a mixture with a total pressure of 6 atm is found using Dalton's Law of Partial Pressures. The result is approximately 2.0 atm, which matches option B.
Step-by-step explanation:
To find the partial pressure of N₂ in a mixture of gases using Dalton's Law, you take the total pressure and multiply it by the mole fraction of the gas. The mole fraction is the ratio of moles of a specific gas to the total moles of the gas mixture. In this case, we have 1.0 mole of N₂ and 2.0 moles of O₂, which makes a total of 3.0 moles of gas.
The mole fraction of N₂ (XN₂) is 1.0 mole of N₂ divided by the total 3.0 moles, which is ⅓ or approximately 0.3333. To find the partial pressure of N₂ (PN₂), we multiply the total pressure of the gas mixture by the mole fraction of N₂:
PN₂ = Total Pressure × XN₂PN₂ = 6 atm × 0.3333
When calculated, the partial pressure of N₂ comes out to be approximately 2.0 atm, which corresponds to option B.