# How do you calculate the partial pressures of this problem?

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A mixture containing 2.53 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a temperature of 25°C.

(a) Calculate the partial pressure of each of the gases in the mixture.

(b) Calculate the total pressure of the mixture.

Answers in atmospheres.

A mixture containing 2.53 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a temperature of 25°C.

(a) Calculate the partial pressure of each of the gases in the mixture.

(b) Calculate the total pressure of the mixture.

Answers in atmospheres.

##### 1 Answer

In a gaseous mixture, the pressure exerted by a component is the same as if it ALONE occupied the container............

#### Explanation:

.........and the total pressure is the sum of the individual partial pressures.

The above was a restatement of Dalton's Law of Partial Pressures, which was a very early experimental finding. From this, to find the pressure exerted by a component, all we need to do is find the total number of moles of each gas, and proceed from there.

In your problem there are

Now we may use Dalton's Law to get the individual partial pressures:

And

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