Final answer:
Using Dalton's Law, the partial pressure of nitrogen (N₂) in the vessel is 0.79 atm, and the partial pressure of oxygen (O₂) is 0.21 atm.
Step-by-step explanation:
The partial pressure of a gas in a mixture can be found using Dalton's Law of Partial Pressures, which states that the total pressure exerted by a gas mixture is the sum of the partial pressures of each individual component gas. These partial pressures are directly proportional to the percentage composition of each gas.
For nitrogen (N₂), which makes up 79% of the air by volume, the partial pressure can be calculated as follows:
Partial pressure of N₂ = Total pressure × Percentage of N₂
= 1.00 atm × 0.79
= 0.79 atm
Therefore, the partial pressure of N₂ is 0.79 atm.
Similarly, for oxygen (O₂), which makes up 21% of the air by volume, the partial pressure is:
Partial pressure of O₂ = Total pressure × Percentage of O₂
= 1.00 atm × 0.21
= 0.21 atm
The partial pressure of O₂ in the air-filled vessel is 0.21 atm.