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Calculate the cell potential of Cu-Fe galvanic cell at the following conditions: i) Standard conditions ii) When 90% of Cu2+ has been consumed

Calculate the cell potential of Cu-Fe galvanic cell at the following conditions: i) Standard conditions ii) When 90% of Cu2+ has been consumed

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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Q1: Calculate the cell potential of Cu-Fe galvanic cell at the following dpan conditions: i) Standard conditions ii) When 90% of Cu2+ has been consumed Q2: Determine the cell potential for the following concentration cell: i) Cr(s) / Cr3+ (0.05M) // Cr3+ (2.0M)/ Cr(s) Zn | Zn2+ (1M) // Zn2+ (1M) | Zn ii) Q3: Calculate the equilibrium constant at 25°C for the reaction between zinc metal and acid. Zn + 2H+ → Zn2+ + H2 Q4: Calculate the solubility product at 25°C for Mg(OH),2. Mg(OH)2 + 2e Mg2+ + 2e > Mg + 20H E° = -2.69 V > Mg E° = -2.38 V Q5: Identify the products at anode and cathode for electrolysis of: i) molten PbCl, salt ii) aqueous Magnesium Sulphate iii) Mixture of molten MgBr + NaCI iv) Mixture solution of MgBr + Nacl A copper electroplating process utilizes 15 A of current by chemically dissolving (corroding) a copper anode and electroplating a copper cathode. If it is assumed that there are no side reactions, how long will it take to corrode 20g of copper from the anode? (Atomic mass of Cu: 64 g/mol) Q6: Calculate the volume of H, gas at 25°C and 1.00 atm that will be collected at the cathode when an aqueous solution of Na,SO, is electrolyzed for 2.00 hours with a 10.0-amp current at 90% current efficiency. Q7: (Hint: use ideal gas law, PV=mRT) R = 0.08205 L.atm/mol.K %3D Determine the oxidation number of the chromium in an unknown salt if electrolysis of a molten sample of this salt for 1.50 hours with a 10.0-amp current deposits 9.71 grams of chromium metal at the cathode. Q8:
Transcribed Image Text:Q1: Calculate the cell potential of Cu-Fe galvanic cell at the following dpan conditions: i) Standard conditions ii) When 90% of Cu2+ has been consumed Q2: Determine the cell potential for the following concentration cell: i) Cr(s) / Cr3+ (0.05M) // Cr3+ (2.0M)/ Cr(s) Zn | Zn2+ (1M) // Zn2+ (1M) | Zn ii) Q3: Calculate the equilibrium constant at 25°C for the reaction between zinc metal and acid. Zn + 2H+ → Zn2+ + H2 Q4: Calculate the solubility product at 25°C for Mg(OH),2. Mg(OH)2 + 2e Mg2+ + 2e > Mg + 20H E° = -2.69 V > Mg E° = -2.38 V Q5: Identify the products at anode and cathode for electrolysis of: i) molten PbCl, salt ii) aqueous Magnesium Sulphate iii) Mixture of molten MgBr + NaCI iv) Mixture solution of MgBr + Nacl A copper electroplating process utilizes 15 A of current by chemically dissolving (corroding) a copper anode and electroplating a copper cathode. If it is assumed that there are no side reactions, how long will it take to corrode 20g of copper from the anode? (Atomic mass of Cu: 64 g/mol) Q6: Calculate the volume of H, gas at 25°C and 1.00 atm that will be collected at the cathode when an aqueous solution of Na,SO, is electrolyzed for 2.00 hours with a 10.0-amp current at 90% current efficiency. Q7: (Hint: use ideal gas law, PV=mRT) R = 0.08205 L.atm/mol.K %3D Determine the oxidation number of the chromium in an unknown salt if electrolysis of a molten sample of this salt for 1.50 hours with a 10.0-amp current deposits 9.71 grams of chromium metal at the cathode. Q8:
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