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## Q. 8.11

Using Dalton’s Law: Finding Partial Pressures

Humid air on a warm summer day is approximately 20% oxygen, 75% nitrogen, 4% water vapor, and 1% argon. What is the partial pressure of each component if the atmospheric pressure is $1.0 ×10^{5} Pa$ ?

ANALYSIS According to Dalton’s law, the partial pressure of any gas in a mixture is equal to the percent concentration of the gas times the total gas pressure (750 mmHg). In this case

$P_{total} = P_{O_{2}} + P_{N_{2}} + P_{H_{2}O} + P_{Ar}$

## Verified Solution

Oxygen partial pressure ( $P_{O_{2}}$ ):                 $0.20 × 10^{5} Pa$

Nitrogen partial pressure ($P_{N_{2}}$  )               $0.75 × 10^{5} Pa$

Water vapor partial pressure ($P_{H_{2}O}$ ):      $0.04 × 10^{5} Pa$

Argon partial pressure ($P_{Ar}$ ):                        $0.01 × 10^{5} Pa$

Total pressure =$1.0 × 10^{5} Pa$

Note that the sum of the partial pressures must equal the total pressure (within rounding error).