Three gases (8.00 g of methane, ch4, 18.0 g of ethane, c2h6, and an unknown amount of propane, c3h8) were added to the same 10.0-l container. at 23.0 ∘c, the total pressure in the container is 5.00 atm . calculate the partial pressure of each gas in the container.

Partial pressure of methane: 1.18 atm

Partial pressure of ethane: 1.45 atm

Partial pressure of propane: 2.35 atm

Explanation:

Let the total moles of gases in a container be n.

Total pressure of the gases in a container =P = 5.0 atm

Temperature of the gases in a container =T = 23°C = 296.15 K

Volume of the container = V = 10.0 L

(Ideal gas equation)

Moles of methane gas =

Moles of ethane gas =

Moles of propane gas =

Partial pressure of all the gases can be calculated by using Raoult's law:

= partial pressure of 'i' component.

= mole fraction of 'i' component in mixture

P = total pressure of the mixture

Partial pressure of methane:

Partial pressure of ethane:

Partial pressure of propane:

i know insulin is primary but i dont know the others im sorry

explanation: