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Use measured cell potential to calculate concentration. When [Ag] 1.18 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 3.283 V. What is the Mg2+ concentration in this cell? 2Ag (aq) + Mg(s)-2Ag(s) + Mg2+(aq) [Mg2+] = 1.84x10^-4 M Calculate quantity of materials produced from the electrolysis of a molten salt. Close Problem A current of 17.3A is passed through an electrolysis cell containing molten MgCl2 for 37.2 minutes. (a) Predict the products of the electrolysis and write the reactions occurring at the anode and cathode. Write electrons as e. Use smallest integer coefficients possible and omit states. If a box is not needed, leave it blank. Cathode reaction: Mg 2+ + 2e" Mg Anode reaction: 2C1- + Cl₂ + 2e (b) Calculate the grams of metal or liters of gas formed at the cathode and anode (assume gases are at 298 K and 1.00 atm). Formed at cathode: 9.75 grams Formed at anode: 0.201 liters

Use measured cell potential to calculate concentration. When [Ag] 1.18 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 3.283 V. What is the Mg2+ concentration in this cell? 2Ag (aq) + Mg(s)-2Ag(s) + Mg2+(aq) [Mg2+] = 1.84x10^-4 M Calculate quantity of materials produced from the electrolysis of a molten salt. Close Problem A current of 17.3A is passed through an electrolysis cell containing molten MgCl2 for 37.2 minutes. (a) Predict the products of the electrolysis and write the reactions occurring at the anode and cathode. Write electrons as e. Use smallest integer coefficients possible and omit states. If a box is not needed, leave it blank. Cathode reaction: Mg 2+ + 2e" Mg Anode reaction: 2C1- + Cl₂ + 2e (b) Calculate the grams of metal or liters of gas formed at the cathode and anode (assume gases are at 298 K and 1.00 atm). Formed at cathode: 9.75 grams Formed at anode: 0.201 liters

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.71QP: What is the standard cell potential you would obtain from a cell at 25C using an electrode in which...
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Use measured cell potential to calculate concentration. When [Ag] 1.18 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 3.283 V. What is the Mg2+ concentration in this cell? 2Ag (aq) + Mg(s)-2Ag(s) + Mg2+(aq) [Mg2+] = 1.84x10^-4 M
Transcribed Image Text:Use measured cell potential to calculate concentration. When [Ag] 1.18 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 3.283 V. What is the Mg2+ concentration in this cell? 2Ag (aq) + Mg(s)-2Ag(s) + Mg2+(aq) [Mg2+] = 1.84x10^-4 M
Calculate quantity of materials produced from the electrolysis of a molten salt. Close Problem A current of 17.3A is passed through an electrolysis cell containing molten MgCl2 for 37.2 minutes. (a) Predict the products of the electrolysis and write the reactions occurring at the anode and cathode. Write electrons as e. Use smallest integer coefficients possible and omit states. If a box is not needed, leave it blank. Cathode reaction: Mg 2+ + 2e" Mg Anode reaction: 2C1- + Cl₂ + 2e (b) Calculate the grams of metal or liters of gas formed at the cathode and anode (assume gases are at 298 K and 1.00 atm). Formed at cathode: 9.75 grams Formed at anode: 0.201 liters
Transcribed Image Text:Calculate quantity of materials produced from the electrolysis of a molten salt. Close Problem A current of 17.3A is passed through an electrolysis cell containing molten MgCl2 for 37.2 minutes. (a) Predict the products of the electrolysis and write the reactions occurring at the anode and cathode. Write electrons as e. Use smallest integer coefficients possible and omit states. If a box is not needed, leave it blank. Cathode reaction: Mg 2+ + 2e" Mg Anode reaction: 2C1- + Cl₂ + 2e (b) Calculate the grams of metal or liters of gas formed at the cathode and anode (assume gases are at 298 K and 1.00 atm). Formed at cathode: 9.75 grams Formed at anode: 0.201 liters
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