Textbook Question
Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor. (b) If the volume of the exhaled gas is 455 mL and its temperature is 37 °C, calculate the number of moles of CO2 exhaled.
7. Gases
Partial Pressure
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A mixture of 10.0 g of Ne and 10.0 g of Ar has a total pressure of 1.60 atm. What is the partial pressure of Ar in the mixture?
A
1.20 atm
B
1.60 atm
C
0.64 atm
D
0.96 atm
Verified step by step guidance1
First, calculate the number of moles of Ne (neon) using its molar mass. The molar mass of Ne is approximately 20.18 g/mol. Use the formula: \( n = \frac{\text{mass}}{\text{molar mass}} \).
Next, calculate the number of moles of Ar (argon) using its molar mass. The molar mass of Ar is approximately 39.95 g/mol. Again, use the formula: \( n = \frac{\text{mass}}{\text{molar mass}} \).
Determine the total number of moles in the mixture by adding the moles of Ne and Ar together.
Use Dalton's Law of Partial Pressures, which states that the partial pressure of a gas in a mixture is proportional to its mole fraction. Calculate the mole fraction of Ar: \( \text{mole fraction of Ar} = \frac{\text{moles of Ar}}{\text{total moles}} \).
Finally, calculate the partial pressure of Ar by multiplying its mole fraction by the total pressure of the mixture: \( P_{\text{Ar}} = \text{mole fraction of Ar} \times \text{total pressure} \).
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