**Problem Statement:** Three gases -- Ar (Argon), N₂ (Nitrogen), and H₂ (Hydrogen) -- are mixed in a 500 L container at 298 K. Ar has a pressure of 255 torr, N₂ has a pressure of 228 torr, and the pressure of H₂ is unknown. If the total pressure in the container is 550 torr, what would be the pressure of the H₂ gas? **Options:** - 295 torr - 67 torr - 483 torr - 17 torr **Explanation:** To find the pressure of H₂, we 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. Given: - Pressure of Ar = 255 torr - Pressure of N₂ = 228 torr - Total Pressure = 550 torr According to Dalton’s Law: \[ \text{Total Pressure} = P_{\text{Ar}} + P_{\text{N}_2} + P_{\text{H}_2} \] \[ 550 \, \text{torr} = 255 \, \text{torr} + 228 \, \text{torr} + P_{\text{H}_2} \] \[ P_{\text{H}_2} = 550 \, \text{torr} - (255 \, \text{torr} + 228 \, \text{torr}) \] \[ P_{\text{H}_2} = 550 \, \text{torr} - 483 \, \text{torr} \] \[ P_{\text{H}_2} = 67 \, \text{torr} \] Thus, the pressure of the \( \text{H}_2 \) gas is 67 torr.
**Problem Statement:** Three gases -- Ar (Argon), N₂ (Nitrogen), and H₂ (Hydrogen) -- are mixed in a 500 L container at 298 K. Ar has a pressure of 255 torr, N₂ has a pressure of 228 torr, and the pressure of H₂ is unknown. If the total pressure in the container is 550 torr, what would be the pressure of the H₂ gas? **Options:** - 295 torr - 67 torr - 483 torr - 17 torr **Explanation:** To find the pressure of H₂, we 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. Given: - Pressure of Ar = 255 torr - Pressure of N₂ = 228 torr - Total Pressure = 550 torr According to Dalton’s Law: \[ \text{Total Pressure} = P_{\text{Ar}} + P_{\text{N}_2} + P_{\text{H}_2} \] \[ 550 \, \text{torr} = 255 \, \text{torr} + 228 \, \text{torr} + P_{\text{H}_2} \] \[ P_{\text{H}_2} = 550 \, \text{torr} - (255 \, \text{torr} + 228 \, \text{torr}) \] \[ P_{\text{H}_2} = 550 \, \text{torr} - 483 \, \text{torr} \] \[ P_{\text{H}_2} = 67 \, \text{torr} \] Thus, the pressure of the \( \text{H}_2 \) gas is 67 torr.
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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how would you solve this? this is a non graded practice
![**Problem Statement:**
Three gases -- Ar (Argon), N₂ (Nitrogen), and H₂ (Hydrogen) -- are mixed in a 500 L container at 298 K. Ar has a pressure of 255 torr, N₂ has a pressure of 228 torr, and the pressure of H₂ is unknown. If the total pressure in the container is 550 torr, what would be the pressure of the H₂ gas?
**Options:**
- 295 torr
- 67 torr
- 483 torr
- 17 torr
**Explanation:**
To find the pressure of H₂, we 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.
Given:
- Pressure of Ar = 255 torr
- Pressure of N₂ = 228 torr
- Total Pressure = 550 torr
According to Dalton’s Law:
\[ \text{Total Pressure} = P_{\text{Ar}} + P_{\text{N}_2} + P_{\text{H}_2} \]
\[ 550 \, \text{torr} = 255 \, \text{torr} + 228 \, \text{torr} + P_{\text{H}_2} \]
\[ P_{\text{H}_2} = 550 \, \text{torr} - (255 \, \text{torr} + 228 \, \text{torr}) \]
\[ P_{\text{H}_2} = 550 \, \text{torr} - 483 \, \text{torr} \]
\[ P_{\text{H}_2} = 67 \, \text{torr} \]
Thus, the pressure of the \( \text{H}_2 \) gas is 67 torr.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6dac1fe8-9484-432e-9121-04aedd30c8dd%2Fcbefd0b2-8832-41d7-88b9-8fa35dee1ebc%2F61ohs3k_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
Three gases -- Ar (Argon), N₂ (Nitrogen), and H₂ (Hydrogen) -- are mixed in a 500 L container at 298 K. Ar has a pressure of 255 torr, N₂ has a pressure of 228 torr, and the pressure of H₂ is unknown. If the total pressure in the container is 550 torr, what would be the pressure of the H₂ gas?
**Options:**
- 295 torr
- 67 torr
- 483 torr
- 17 torr
**Explanation:**
To find the pressure of H₂, we 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.
Given:
- Pressure of Ar = 255 torr
- Pressure of N₂ = 228 torr
- Total Pressure = 550 torr
According to Dalton’s Law:
\[ \text{Total Pressure} = P_{\text{Ar}} + P_{\text{N}_2} + P_{\text{H}_2} \]
\[ 550 \, \text{torr} = 255 \, \text{torr} + 228 \, \text{torr} + P_{\text{H}_2} \]
\[ P_{\text{H}_2} = 550 \, \text{torr} - (255 \, \text{torr} + 228 \, \text{torr}) \]
\[ P_{\text{H}_2} = 550 \, \text{torr} - 483 \, \text{torr} \]
\[ P_{\text{H}_2} = 67 \, \text{torr} \]
Thus, the pressure of the \( \text{H}_2 \) gas is 67 torr.
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