Question

question 6 of 30
a mixture of he, ne, and n₂ gases has a pressure of 1.943 atm. if the
pressures of he and ne are 0.137 atm and 0.566 atm, respectively, what is
the partial pressure of n₂ in the mixture?

a. 1.24 atm

b. 1.943 atm

c. 0.151 atm

d. 0.703 atm

Explanation:

Step1: Recall Dalton's Law of Partial Pressures

Dalton's Law states that the total pressure \( P_{\text{total}} \) of a gas mixture is the sum of the partial pressures of its components. So, \( P_{\text{total}} = P_{\text{He}} + P_{\text{Ne}} + P_{\text{N}_2} \).

Step2: Rearrange the formula to solve for \( P_{\text{N}_2} \)

We can rearrange the formula to \( P_{\text{N}_2} = P_{\text{total}} - P_{\text{He}} - P_{\text{Ne}} \).

Step3: Substitute the given values

Given \( P_{\text{total}} = 1.943 \) atm, \( P_{\text{He}} = 0.137 \) atm, and \( P_{\text{Ne}} = 0.566 \) atm. Substitute these values into the formula:
\( P_{\text{N}_2} = 1.943 - 0.137 - 0.566 \)

Step4: Perform the arithmetic

First, calculate \( 0.137 + 0.566 = 0.703 \). Then, \( 1.943 - 0.703 = 1.24 \) atm.

Answer:

A. 1.24 atm