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Table 1. Mass calculations for copper electrode. Mass of copper (initial) (g) Mass of copper (final) (g) Mass of copper oxidized (g) 1. Table 2. Record of current (measured in amps) and time (measured in minutes) as they changed throughout the experiment. 0 3 6 9 Complete the following table: Table 3. Summary of observation data. 2.4622 Time Current Time Current Time 24 0.154 12 15 0.153 27 18 0.152 30 21 0.152 33 0.157 0.156 0.155 0.155 Data Analysis: 2.3269 0.135 Total reaction time (s) Average current (A) Volume of H, produced (mL) Barometric pressure (kPa) Partial pressure of water vapour (kPa) Partial pressure of H₂ al produced (kPa) Temperature (°C) Current Time Current 0.151 36 0.151 39 0.150 42 0.149 45 50.00 101.40 3.19 25.00 0.148 0.148 0.147 0.146 Show how you calculated the partial pressure of the hydrogen gas that was produced. 2. Determine the number of mols of H₂ gas produced using the ideal gas law. R = 8.314 kPa L mol-¹K-¹ (1) (2) Based on the anode information (3) (1) (1) 3. Determine the number of mols of electrons required to produce the amount of hydrogen you collected. (1) 4. Determine the number of mols of Cut that were oxidized based on the Cu electrode. (1) 5. Determine the value of n in Cunt based on the above information. Round to the nearest whole number. (4) (1) 6. Determine the number of mols of electrons produced at the anode. 7. Determine the number of Coulombs delivered over the span of the experiment. Calculate the value of Faraday's Constant Based on the cathode information (1) 8. Compare the two values that you calculated with the accepted value of the Faraday. Which of your measured results is the more accurate. Give an experimental reason why this may be. (3)

Table 1. Mass calculations for copper electrode. Mass of copper (initial) (g) Mass of copper (final) (g) Mass of copper oxidized (g) 1. Table 2. Record of current (measured in amps) and time (measured in minutes) as they changed throughout the experiment. 0 3 6 9 Complete the following table: Table 3. Summary of observation data. 2.4622 Time Current Time Current Time 24 0.154 12 15 0.153 27 18 0.152 30 21 0.152 33 0.157 0.156 0.155 0.155 Data Analysis: 2.3269 0.135 Total reaction time (s) Average current (A) Volume of H, produced (mL) Barometric pressure (kPa) Partial pressure of water vapour (kPa) Partial pressure of H₂ al produced (kPa) Temperature (°C) Current Time Current 0.151 36 0.151 39 0.150 42 0.149 45 50.00 101.40 3.19 25.00 0.148 0.148 0.147 0.146 Show how you calculated the partial pressure of the hydrogen gas that was produced. 2. Determine the number of mols of H₂ gas produced using the ideal gas law. R = 8.314 kPa L mol-¹K-¹ (1) (2) Based on the anode information (3) (1) (1) 3. Determine the number of mols of electrons required to produce the amount of hydrogen you collected. (1) 4. Determine the number of mols of Cut that were oxidized based on the Cu electrode. (1) 5. Determine the value of n in Cunt based on the above information. Round to the nearest whole number. (4) (1) 6. Determine the number of mols of electrons produced at the anode. 7. Determine the number of Coulombs delivered over the span of the experiment. Calculate the value of Faraday's Constant Based on the cathode information (1) 8. Compare the two values that you calculated with the accepted value of the Faraday. Which of your measured results is the more accurate. Give an experimental reason why this may be. (3)

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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Table 1. Mass calculations for copper electrode. Mass of copper (initial) (g) Mass of copper (final) (g) Mass of copper oxidized (g) 1. Table 2. Record of current (measured in amps) and time (measured in minutes) as they changed throughout the experiment. 0 3 6 9 Complete the following table: Table 3. Summary of observation data. 2.4622 Time Current Time Current Time 24 0.154 12 15 0.153 27 18 0.152 30 21 0.152 33 0.157 0.156 0.155 0.155 Data Analysis: 2.3269 0.135 Total reaction time (s) Average current (A) Volume of H, produced (mL) Barometric pressure (kPa) Partial pressure of water vapour (kPa) Partial pressure of H₂ al produced (kPa) Temperature (°C) Current Time Current 0.151 36 0.151 39 0.150 42 0.149 45 50.00 101.40 3.19 25.00 0.148 0.148 0.147 0.146 Show how you calculated the partial pressure of the hydrogen gas that was produced. 2. Determine the number of mols of H₂ gas produced using the ideal gas law. R = 8.314 kPa L mol-¹K-¹ (1) (2) Based on the anode information (3) (1) (1) 3. Determine the number of mols of electrons required to produce the amount of hydrogen you collected. (1) 4. Determine the number of mols of Cut that were oxidized based on the Cu electrode. (1) 5. Determine the value of n in Cunt based on the above information. Round to the nearest whole number. (4) (1) 6. Determine the number of mols of electrons produced at the anode. 7. Determine the number of Coulombs delivered over the span of the experiment. Calculate the value of Faraday's Constant Based on the cathode information (1) 8. Compare the two values that you calculated with the accepted value of the Faraday. Which of your measured results is the more accurate. Give an experimental reason why this may be. (3)
Transcribed Image Text:Table 1. Mass calculations for copper electrode. Mass of copper (initial) (g) Mass of copper (final) (g) Mass of copper oxidized (g) 1. Table 2. Record of current (measured in amps) and time (measured in minutes) as they changed throughout the experiment. 0 3 6 9 Complete the following table: Table 3. Summary of observation data. 2.4622 Time Current Time Current Time 24 0.154 12 15 0.153 27 18 0.152 30 21 0.152 33 0.157 0.156 0.155 0.155 Data Analysis: 2.3269 0.135 Total reaction time (s) Average current (A) Volume of H, produced (mL) Barometric pressure (kPa) Partial pressure of water vapour (kPa) Partial pressure of H₂ al produced (kPa) Temperature (°C) Current Time Current 0.151 36 0.151 39 0.150 42 0.149 45 50.00 101.40 3.19 25.00 0.148 0.148 0.147 0.146 Show how you calculated the partial pressure of the hydrogen gas that was produced. 2. Determine the number of mols of H₂ gas produced using the ideal gas law. R = 8.314 kPa L mol-¹K-¹ (1) (2) Based on the anode information (3) (1) (1) 3. Determine the number of mols of electrons required to produce the amount of hydrogen you collected. (1) 4. Determine the number of mols of Cut that were oxidized based on the Cu electrode. (1) 5. Determine the value of n in Cunt based on the above information. Round to the nearest whole number. (4) (1) 6. Determine the number of mols of electrons produced at the anode. 7. Determine the number of Coulombs delivered over the span of the experiment. Calculate the value of Faraday's Constant Based on the cathode information (1) 8. Compare the two values that you calculated with the accepted value of the Faraday. Which of your measured results is the more accurate. Give an experimental reason why this may be. (3)
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