**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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