What is the partial pressure of He in a balloon that is filled with 0.676 moles of He 0.075 moles of N₂. and 0.085 moles of O₂ to a total pressure of 0.30 atm? (Give your answer to 2 decimal places and no units)
What is the partial pressure of He in a balloon that is filled with 0.676 moles of He 0.075 moles of N₂. and 0.085 moles of O₂ to a total pressure of 0.30 atm? (Give your answer to 2 decimal places and no units)
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Question:**
What is the partial pressure of He in a balloon that is filled with 0.676 moles of He, 0.075 moles of N₂, and 0.085 moles of O₂ to a total pressure of 0.30 atm? (Give your answer to 2 decimal places and no units.)
**Solution Explanation:**
To calculate the partial pressure of He, we will use Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. The partial pressure of a gas can be calculated using the mole fraction of the gas and the total pressure:
1. **Calculate the total number of moles in the mixture:**
\[
\text{Total moles} = \text{moles of He} + \text{moles of N}_2 + \text{moles of O}_2
\]
\[
\text{Total moles} = 0.676 + 0.075 + 0.085 = 0.836 \text{ moles}
\]
2. **Calculate the mole fraction of He:**
\[
\text{Mole fraction of He} = \frac{\text{moles of He}}{\text{Total moles}} = \frac{0.676}{0.836}
\]
3. **Calculate the partial pressure of He:**
\[
\text{Partial pressure of He} = \text{Mole fraction of He} \times \text{Total pressure}
\]
\[
\text{Partial pressure of He} = \left(\frac{0.676}{0.836}\right) \times 0.30
\]
Finally, calculate to find the partial pressure and round to two decimal places, providing the answer without units.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffc7deb2c-0862-415e-88b2-023e0d274874%2F8fed4f8d-17a7-4055-a9e3-73a62f60f5a5%2Flvvm9qn_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
What is the partial pressure of He in a balloon that is filled with 0.676 moles of He, 0.075 moles of N₂, and 0.085 moles of O₂ to a total pressure of 0.30 atm? (Give your answer to 2 decimal places and no units.)
**Solution Explanation:**
To calculate the partial pressure of He, we will use Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. The partial pressure of a gas can be calculated using the mole fraction of the gas and the total pressure:
1. **Calculate the total number of moles in the mixture:**
\[
\text{Total moles} = \text{moles of He} + \text{moles of N}_2 + \text{moles of O}_2
\]
\[
\text{Total moles} = 0.676 + 0.075 + 0.085 = 0.836 \text{ moles}
\]
2. **Calculate the mole fraction of He:**
\[
\text{Mole fraction of He} = \frac{\text{moles of He}}{\text{Total moles}} = \frac{0.676}{0.836}
\]
3. **Calculate the partial pressure of He:**
\[
\text{Partial pressure of He} = \text{Mole fraction of He} \times \text{Total pressure}
\]
\[
\text{Partial pressure of He} = \left(\frac{0.676}{0.836}\right) \times 0.30
\]
Finally, calculate to find the partial pressure and round to two decimal places, providing the answer without units.
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