Question

A gas mixture contains an equal number of moles of He and Ne
The total pressure of the mixture is 6.0 atm

What is the partial pressure of He?

What is the partial pressure of Ne?

Answer 1

Answer:

$\large \boxed{\text{3.0 atm; 3.0 atm}}$

Explanation:

We can use Dalton's Law of Partial Pressures:

Each gas in a mixture of gases equals its pressure separately from the other gases.

If the molecules of a gas make up one-half of the mixture, the partial pressure is one-half of the total pressure.

$p_{\text{He}} = p_{\text{tot}} \times \dfrac{\text{1 part He}}{\text{2 parts total}}= \text{6.0 atm} \times \dfrac{1}{2} = \textbf{3.0 atm}\\\\p_{\text{Ne}} = p_{\text{tot}} \times \dfrac{\text{1 part Ne}}{\text{2 parts total}}= \text{6.0 atm} \times \dfrac{1}{2} = \textbf{3.0 atm}\\\\\text{The partial pressure of each gas is \large \boxed{\textbf{3.0 atm}} }$

Answer 2

The partial pressures of the He and Ne gases which make up the gas mixture are; 3.0atm and 3.0atm respectively.

Definition:

By Dalton's law of partial pressure ; the total pressure of a mixture of gases occupying a given volume is equal to the sum of the partial pressures of each gas, considered separately, at constant temperature.

According to the question;

The total pressure of the mixture is 6.0 atm.

The partial pressure of He is;

• P(He) = (1/2) × 6.0 atm

P(He) = 3.0 atm

The partial pressure of Ne is;

• P(Ne) = (1/2) × 6.0 atm

P(Ne) = 3.0 atm

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