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Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. Y Part A What is the partial pressure of nitrogen in air at atmospheric pressure (1 atm)? Assume ideal behavior. Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) Value Submit HA Part B Complete previous part(s) ▾ Part C PA Units What is the partial pressure of oxygen in air at atmospheric pressure (1 atm)? Assume ideal behavior. Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) Value ? Units

Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. Y Part A What is the partial pressure of nitrogen in air at atmospheric pressure (1 atm)? Assume ideal behavior. Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) Value Submit HA Part B Complete previous part(s) ▾ Part C PA Units What is the partial pressure of oxygen in air at atmospheric pressure (1 atm)? Assume ideal behavior. Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) Value ? Units

Chemistry
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Answer part a and b
**Educational Website Transcription:** --- ### Understanding Gas Mixtures and Partial Pressures #### Overview: Air is composed predominantly of nitrogen and oxygen, with approximately 78.0% nitrogen molecules and 21.0% oxygen molecules. Other gases make up the remaining 1% of air molecules. #### Ideal Gas Law: The ideal gas law is expressed as: \[ PV = nRT \] This law indicates that pressure (\( P \)) is independent of the type of gas present. The pressure exerted by a mixture of gases is the sum of the pressures that each gas would individually exert. #### Dalton’s Law of Partial Pressures: In a mixture of gases, the total pressure is the sum of the partial pressures of each gas present: \[ P_{\text{total}} = P_1 + P_2 + P_3 + \ldots \] Each partial pressure (\( P_i \)) is calculated as if the respective gas were occupying the entire volume alone: \[ P_i = \frac{n_iRT}{V} \] #### Homework Problems: - **Part A:** What is the partial pressure of nitrogen in air at atmospheric pressure (1 atm)? Assume ideal behavior. - **Response Format:** Express your answer to three significant figures with appropriate units. - **Part C:** What is the partial pressure of oxygen in air at atmospheric pressure (1 atm)? Assume ideal behavior. - **Response Format:** Express your answer to three significant figures with appropriate units. ### Instructions: - Enter the calculated value and unit for each part in the provided fields. - Select "Submit" to record your answers. --- **Note:** To understand the behaviors of individual gases in mixtures, assume ideal gas conditions under which gases follow the ideal gas law closely, especially at high temperatures and low pressures.
Transcribed Image Text:**Educational Website Transcription:** --- ### Understanding Gas Mixtures and Partial Pressures #### Overview: Air is composed predominantly of nitrogen and oxygen, with approximately 78.0% nitrogen molecules and 21.0% oxygen molecules. Other gases make up the remaining 1% of air molecules. #### Ideal Gas Law: The ideal gas law is expressed as: \[ PV = nRT \] This law indicates that pressure (\( P \)) is independent of the type of gas present. The pressure exerted by a mixture of gases is the sum of the pressures that each gas would individually exert. #### Dalton’s Law of Partial Pressures: In a mixture of gases, the total pressure is the sum of the partial pressures of each gas present: \[ P_{\text{total}} = P_1 + P_2 + P_3 + \ldots \] Each partial pressure (\( P_i \)) is calculated as if the respective gas were occupying the entire volume alone: \[ P_i = \frac{n_iRT}{V} \] #### Homework Problems: - **Part A:** What is the partial pressure of nitrogen in air at atmospheric pressure (1 atm)? Assume ideal behavior. - **Response Format:** Express your answer to three significant figures with appropriate units. - **Part C:** What is the partial pressure of oxygen in air at atmospheric pressure (1 atm)? Assume ideal behavior. - **Response Format:** Express your answer to three significant figures with appropriate units. ### Instructions: - Enter the calculated value and unit for each part in the provided fields. - Select "Submit" to record your answers. --- **Note:** To understand the behaviors of individual gases in mixtures, assume ideal gas conditions under which gases follow the ideal gas law closely, especially at high temperatures and low pressures.
Expert Solution
Step 1: Dalton's law of partial pressure

Answer:

According to Dalton's law of partial pressure, partial pressure of a gas in a system is equal to the product of mole fraction and total pressure, so

straight P subscript gas equals straight y subscript gas cross times straight P subscript total

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