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Use your balanced redox reaction to calculate the moles of your metal, Mt, that oxidized.

Use your balanced redox reaction to calculate the moles of your metal, Mt, that oxidized.

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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LAB-9: Molar Mass by Electrolysis Attach the other end of the copper s-hook's alligator clip to the negative end of the DC power supply. Hydrogen gas should begin to evolve in the burette. Monitor the gas collection, and unhook the anode metal from the power supply when the level in the burette is about 45 mL. 6. 7. Measure the volume level within the burette. Record in the data table as the Final Volume. 8. Rinse the metal anode with 0.5 M HC₂H3CO2, then rinse with water, and then alcohol. Let the metal air-dry. Measure and record the mass of the metal anode to +0.0001 g, and record as Final Mass of the Metal Anode. 9. Complete your data table by calculating all missing values. Record the values and units in the data table. 10. Clean and stow all equipment. Dispose of your solutions according to your instructor's directions. Analysis/Conclusions 1. Using your data, calculate the moles of hydrogen gas, H₂, produced. PV RT =n →n= n = 1.829 mol H₂ 2. a. Write the balanced equation for the 2-reaction for the reduction of H¹+ to H₂. b. Write the balanced equation for the 2-reaction for the oxidation of your metal, Mt to Mt²+. C. Name: DATA TABLE Temperature (709.9 mmHg) (48.402) (62-37 mm Hg.L) (301-15k) mol-K Total Pressure Water Vapor Pressure Hydrogen Gas Pressure Initial Volume Final Volume Volume of hydrogen gas Initial Mass of the Metal Anode Final Mass of the metal anode Mass lost by the metal anode Create the balanced redox reaction, by adding your ½ - reactions. 3. Use your balanced redox reaction to calculate the moles of your metal, Mt, that oxidized. 4. Calculate the molar mass, g/mol, of your unknown metal. 28.°C 738-2 mmHg 28-3 mmHg 109.9 mm H₂ 0.20 ml 2H+ + 2e--> H₂ M ->m++c-12M ->2M+ +2e= 2m + 2H+-> 2m+ + H₂ 5. What is the most reasonable identity of your unknown metal. Explain. 48.60 ml 48.40 ml 2-0110 g 1-88549 0.12569 Extension 6. Use Faraday's constant and the moles of hydrogen gas to calculate the coulombs, C, of electric charge transferred.
Transcribed Image Text:LAB-9: Molar Mass by Electrolysis Attach the other end of the copper s-hook's alligator clip to the negative end of the DC power supply. Hydrogen gas should begin to evolve in the burette. Monitor the gas collection, and unhook the anode metal from the power supply when the level in the burette is about 45 mL. 6. 7. Measure the volume level within the burette. Record in the data table as the Final Volume. 8. Rinse the metal anode with 0.5 M HC₂H3CO2, then rinse with water, and then alcohol. Let the metal air-dry. Measure and record the mass of the metal anode to +0.0001 g, and record as Final Mass of the Metal Anode. 9. Complete your data table by calculating all missing values. Record the values and units in the data table. 10. Clean and stow all equipment. Dispose of your solutions according to your instructor's directions. Analysis/Conclusions 1. Using your data, calculate the moles of hydrogen gas, H₂, produced. PV RT =n →n= n = 1.829 mol H₂ 2. a. Write the balanced equation for the 2-reaction for the reduction of H¹+ to H₂. b. Write the balanced equation for the 2-reaction for the oxidation of your metal, Mt to Mt²+. C. Name: DATA TABLE Temperature (709.9 mmHg) (48.402) (62-37 mm Hg.L) (301-15k) mol-K Total Pressure Water Vapor Pressure Hydrogen Gas Pressure Initial Volume Final Volume Volume of hydrogen gas Initial Mass of the Metal Anode Final Mass of the metal anode Mass lost by the metal anode Create the balanced redox reaction, by adding your ½ - reactions. 3. Use your balanced redox reaction to calculate the moles of your metal, Mt, that oxidized. 4. Calculate the molar mass, g/mol, of your unknown metal. 28.°C 738-2 mmHg 28-3 mmHg 109.9 mm H₂ 0.20 ml 2H+ + 2e--> H₂ M ->m++c-12M ->2M+ +2e= 2m + 2H+-> 2m+ + H₂ 5. What is the most reasonable identity of your unknown metal. Explain. 48.60 ml 48.40 ml 2-0110 g 1-88549 0.12569 Extension 6. Use Faraday's constant and the moles of hydrogen gas to calculate the coulombs, C, of electric charge transferred.
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