Answer: The partial pressure of individual components in the container will be same, that is

Step-by-step explanation:
To calculate the total pressure, we use the equation given by ideal gas equation:

where,
P = pressure of the gas
V = Volume of gas = 10.0 L
n = Number of moles =

R = Gas constant =

T = temperature of the gas =
![25^oC=[25+273]K=298K](https://img.qammunity.org/2021/formulas/chemistry/college/h90rloyf77jo1jed7el4n760wq4iuiuecg.png)
Putting values in above equation, we get:

The partial pressure of a gas is given by Raoult's law, which is:
......(1)
where,
= partial pressure of substance A
= total pressure
= mole fraction of substance A
To calculate the mole fraction of a substance, we use the equation:
.......(2)
We are given:
Moles of methane = 0.5 moles
Moles of hydrogen = 0.5 moles
Moles of sulfur dioxide = 0.5 moles
Using equation 2, we get:

Using equation 1, we get:

Partial pressure of methane = 1.22 atm
Using equation 2, we get:

Using equation 1, we get:

Partial pressure of hydrogen gas = 1.22 atm
Using equation 2, we get:

Using equation 1, we get:

Partial pressure of sulfur dioxide = 1.22 atm
Hence, the partial pressure of individual components in the container will be same, that is
