A mixture of 3.05-atm N₂(g) and 5.29-atm He(g) exerts a total pressure of 8.34 atm.
<h3>What does Dalton's law of partial pressure state?</h3>
Dalton's law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
A mixture of N₂(g) and He(g) exerts a total pressure of 8.34 atm, while the partial pressure of N₂ is 3.05 atm.
We will use Dalton's law to calculate the partial pressure of He.
P = pHe + pN₂
pHe = P - pHe = 8.34 atm - 3.05 atm = 5.29 atm
where,
- P is the total pressure.
- pHe is the partial pressure of He.
- pN₂ is the partial pressure of N₂.
A mixture of 3.05-atm N₂(g) and 5.29-atm He(g) exerts a total pressure of 8.34 atm.
Learn more about Dalton's law here: brainly.com/question/14119417
