Question

There is a mixture of 4 moles of hydrogen gas, 8 moles of oxygen, 12 moles of helium, and 6 moles of nitrogen in a closed container. If the pressure of the gas in the container is 7.5 atm, what is the partial pressure of each gas in the container?

Answer 1

`\begin{gathered} Hydrogen\text{ = 1 atm} \\ Oxygen\text{ = 2 atm} \\ Helium\text{ = 3 atm} \\ Nitrogen\text{ = 1.5 atm} \end{gathered}`

Step-by-step explanation:

Here, we want to get the partial pressure of each gas in the container

According to Dalton's law of partial pressure, the total pressure is the sum of the partial pressures of the individual component gases

Mathematically:

`P_T\text{ = P}_1\text{ + P}_2\text{ + P}_3\text{ +... + P}_n`

Now, to calculate for each of the gases, we divide the number of moles of the particular gas by the total number of moles and multiply by the total pressure in the container

The total number of moles will be:

`4\text{ + 8 + 12 + 6 = 30 moles}`

For hydrogen:

`(4)/(30)*7.5\text{ = 1 atm}`

For oxygen:

`(8)/(30)*7.5\text{ = 2 atm}`

For helium:

`(12)/(30)*7.5\text{ = 3 atm}`

For Nitrogen:

`(6)/(30)*7.5\text{ = 1.5 atm}`