A galvanic cell consists of a nickel cathode immersed in a NISO4 solution and a manganese anode immersed in a MnSO4 solution. A salt bridge connects the two half-cells. (a) Write a balanced equation for the cell reaction. + (b) A current of 1.42 A is observed to flow for a period of 1.93 hours. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to? (c) Calculate the change in mass of the nickel electrode. + (d) Calculate the change in mass of the manganese electrode. g is gis C mol
A galvanic cell consists of a nickel cathode immersed in a NISO4 solution and a manganese anode immersed in a MnSO4 solution. A salt bridge connects the two half-cells. (a) Write a balanced equation for the cell reaction. + (b) A current of 1.42 A is observed to flow for a period of 1.93 hours. How much charge passes through the circuit during this time? How many moles of electrons is this charge equivalent to? (c) Calculate the change in mass of the nickel electrode. + (d) Calculate the change in mass of the manganese electrode. g is gis C mol
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.9: Corrosion: Redox Reactions In The Environment
Problem 2.5ACP: Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in...
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please do a,b,c,d i need all answers please
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