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Molar Volume of a Gas Room temperature (T2): 21.4 °C Barometric pressure: 756.6 torr Data Trial 1 Trial 2 Trial 3 Mass of Mg strip .054 g .058 g .053 g Temperature of water in the 600-mL beaker 20.1°C 20.3°C 20.0°C Vapor pressure of water at the temperature in the 600-mL beaker A torr torr WM torr 17.660 17.879 17.552 Volume of gas collected at room temperature 55.2 mL 58.3 mL 54.3 mL Volume of gas in liters (V2) .0552 L .0583 L .0543 L Calculations 1. Partial pressure of hydrogen gas at room torr torr torr temperature 2. Partial pressure of hydrogen gas in atm (P2) atm atm atm 3. Volume of hydrogen gas at STP PSTPVSTP. = P2V2 (solve for VSTP) TSTP %3D T2 mol mol mol 4. Moles of hydrogen produced based on amount of Mg used (use balanced equation)

Molar Volume of a Gas Room temperature (T2): 21.4 °C Barometric pressure: 756.6 torr Data Trial 1 Trial 2 Trial 3 Mass of Mg strip .054 g .058 g .053 g Temperature of water in the 600-mL beaker 20.1°C 20.3°C 20.0°C Vapor pressure of water at the temperature in the 600-mL beaker A torr torr WM torr 17.660 17.879 17.552 Volume of gas collected at room temperature 55.2 mL 58.3 mL 54.3 mL Volume of gas in liters (V2) .0552 L .0583 L .0543 L Calculations 1. Partial pressure of hydrogen gas at room torr torr torr temperature 2. Partial pressure of hydrogen gas in atm (P2) atm atm atm 3. Volume of hydrogen gas at STP PSTPVSTP. = P2V2 (solve for VSTP) TSTP %3D T2 mol mol mol 4. Moles of hydrogen produced based on amount of Mg used (use balanced equation)

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 of hydrogen gas at room temperature. Calculation #1 on image attached. All the data should be there. 

Molar Volume of a Gas Room temperature (T2): 21.4 °C Barometric pressure: 756.6 torr Data Trial 1 Trial 2 Trial 3 Mass of Mg strip .054 g .058 g .053 g Temperature of water in the 600-mL beaker 20.1°C 20.3°C 20.0°C Vapor pressure of water at the temperature in the 600-mL beaker A torr torr WM torr 17.660 17.879 17.552 Volume of gas collected at room temperature 55.2 mL 58.3 mL 54.3 mL Volume of gas in liters (V2) .0552 L .0583 L .0543 L Calculations 1. Partial pressure of hydrogen gas at room torr torr torr temperature 2. Partial pressure of hydrogen gas in atm (P2) atm atm atm 3. Volume of hydrogen gas at STP PSTPVSTP. = P2V2 (solve for VSTP) TSTP %3D T2 mol mol mol 4. Moles of hydrogen produced based on amount of Mg used (use balanced equation)
Transcribed Image Text:Molar Volume of a Gas Room temperature (T2): 21.4 °C Barometric pressure: 756.6 torr Data Trial 1 Trial 2 Trial 3 Mass of Mg strip .054 g .058 g .053 g Temperature of water in the 600-mL beaker 20.1°C 20.3°C 20.0°C Vapor pressure of water at the temperature in the 600-mL beaker A torr torr WM torr 17.660 17.879 17.552 Volume of gas collected at room temperature 55.2 mL 58.3 mL 54.3 mL Volume of gas in liters (V2) .0552 L .0583 L .0543 L Calculations 1. Partial pressure of hydrogen gas at room torr torr torr temperature 2. Partial pressure of hydrogen gas in atm (P2) atm atm atm 3. Volume of hydrogen gas at STP PSTPVSTP. = P2V2 (solve for VSTP) TSTP %3D T2 mol mol mol 4. Moles of hydrogen produced based on amount of Mg used (use balanced equation)
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