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I mix 9.18 grams of nitrogen, 1.68 grams of hydrogen and 1.05 grams of helium in a flask. If the total pressure in the system was found to be 137 kPa. How much pressure of the total does each gas exert? a) The pressure due to the hydrogen was 0.721 Submit Answer Incorrect. Tries 4/99 Previous Tries b) The pressure due to the nitrogen was 0.453atm Submit Answer Incorrect. Tries 2/99 Previous Tries 27 c) The pressure due to the helium was 0.181 Submit Answer Incorrect. Tries 1/99 Previous Tries

I mix 9.18 grams of nitrogen, 1.68 grams of hydrogen and 1.05 grams of helium in a flask. If the total pressure in the system was found to be 137 kPa. How much pressure of the total does each gas exert? a) The pressure due to the hydrogen was 0.721 Submit Answer Incorrect. Tries 4/99 Previous Tries b) The pressure due to the nitrogen was 0.453atm Submit Answer Incorrect. Tries 2/99 Previous Tries 27 c) The pressure due to the helium was 0.181 Submit Answer Incorrect. Tries 1/99 Previous Tries

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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Partial pressure. I don’t know what else to do, I converted total kPa to atm and used the mole fraction of each gas to get the partial pressure for each in atm.
Title: Calculating Partial Pressures in a Gas Mixture Description: This exercise involves calculating the partial pressures exerted by individual gases in a mixture. Given the masses of nitrogen, hydrogen, and helium in a flask, and knowing the total pressure of the system, you must determine the pressure each gas contributes. Problem Statement: You mix 9.18 grams of nitrogen, 1.68 grams of hydrogen, and 1.05 grams of helium in a flask. If the total pressure in the system is determined to be 137 kPa, how much of the total pressure does each gas exert? Calculate the following: a) The pressure due to the hydrogen: - Attempted Answer: 0.721 (Incorrect) - Number of Attempts: 4/99 b) The pressure due to the nitrogen: - Attempted Answer: 0.453 atm (Incorrect) - Number of Attempts: 2/99 c) The pressure due to the helium: - Attempted Answer: 0.181 (Incorrect) - Number of Attempts: 1/99 Note: - Pay attention to the units when calculating pressures. - Review the concept of partial pressures and how they relate to the total pressure and individual gas quantities.
Transcribed Image Text:Title: Calculating Partial Pressures in a Gas Mixture Description: This exercise involves calculating the partial pressures exerted by individual gases in a mixture. Given the masses of nitrogen, hydrogen, and helium in a flask, and knowing the total pressure of the system, you must determine the pressure each gas contributes. Problem Statement: You mix 9.18 grams of nitrogen, 1.68 grams of hydrogen, and 1.05 grams of helium in a flask. If the total pressure in the system is determined to be 137 kPa, how much of the total pressure does each gas exert? Calculate the following: a) The pressure due to the hydrogen: - Attempted Answer: 0.721 (Incorrect) - Number of Attempts: 4/99 b) The pressure due to the nitrogen: - Attempted Answer: 0.453 atm (Incorrect) - Number of Attempts: 2/99 c) The pressure due to the helium: - Attempted Answer: 0.181 (Incorrect) - Number of Attempts: 1/99 Note: - Pay attention to the units when calculating pressures. - Review the concept of partial pressures and how they relate to the total pressure and individual gas quantities.
Expert Solution
Step 1

Given that :

The mass of nitrogen gas (N2) = 9.18 g

The mass of hydrogen gas (H2) = 1.68 g

The mass of helium gas (He) = 1.05 g

Total pressure = 137 kPa

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