Question

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part a
a gas mixture contains each of the following gases at the indicated partial pressure.
what is the total pressure of the mixture?
express your answer in grams per mole to three significant figures.
co₂ 428 mm hg
ar 108 mm hg
o₂ 166 mm hg
h₂ 59 mm hg
p_total = mm hg

Explanation:

Step1: Recall Dalton's Law

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

Step2: Substitute the values

Given $P_{\text{CO}_2} = 428\ \text{mm Hg}$, $P_{\text{Ar}} = 108\ \text{mm Hg}$, $P_{\text{O}_2} = 166\ \text{mm Hg}$, $P_{\text{H}_2} = 59\ \text{mm Hg}$.
Substitute into the formula:
$P_{\text{total}} = 428 + 108 + 166 + 59$.
Calculate the sum: $428 + 108 = 536$; $536 + 166 = 702$; $702 + 59 = 761$.

Answer:

$761\ \text{mm Hg}$