Question

part a
a mixture of he, ar, and xe has a total pressure of 2.30 atm. what is the partial pressure of xe?
the partial pressure of he is 0.350 atm, and the partial pressure of ar is 0.200 atm.
express your answer to three significant figures and include the appropriate units.
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part b
a volume of 18.0 l contains a mixture of 0.250 mole n₂, 0.250 mole o₂, and an unknown quantity of he. the temperature of the mixture is...

Explanation:

Step1: Recall Dalton's Law

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: \( P_{\text{total}} = P_{\text{He}} + P_{\text{Ar}} + P_{\text{Xe}} \).

Step2: Rearrange the formula

To find \( P_{\text{Xe}} \), rearrange the formula: \( P_{\text{Xe}} = P_{\text{total}} - P_{\text{He}} - P_{\text{Ar}} \).

Step3: Substitute the values

Given \( P_{\text{total}} = 2.30 \, \text{atm} \), \( P_{\text{He}} = 0.350 \, \text{atm} \), and \( P_{\text{Ar}} = 0.200 \, \text{atm} \). Substitute these into the formula:
\( P_{\text{Xe}} = 2.30 - 0.350 - 0.200 \).

Step4: Calculate the result

First, \( 2.30 - 0.350 = 1.95 \). Then, \( 1.95 - 0.200 = 1.75 \). So, \( P_{\text{Xe}} = 1.75 \, \text{atm} \) (to three significant figures).

Answer:

\( 1.75 \, \text{atm} \)