A total of 1.855 F of electricity (1 F = 1 mol e") was required to electrodeposit all of the Zn and Co from a solution of ZnSo, and CoSO,. The mixture of Zn and Co that was deposited had a mass of 56.28 g. Calculate the masses of ZnSO, and CoSO, present in the original solution. %3D mass of ZnSO,: mass of COSO

A total of 1.855 F of electricity (1 F = 1 mol e") was required to electrodeposit all of the Zn and Co from a solution of ZnSo, and CoSO,. The mixture of Zn and Co that was deposited had a mass of 56.28 g. Calculate the masses of ZnSO, and CoSO, present in the original solution. %3D mass of ZnSO,: mass of COSO

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 3P

See similar textbooks

Similar questions

Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
Why would a sacrificial anode made of lithium metal be a bad choice despite its ELi+/Li=2.07V, which appears to be able to protect all the other metals listed in the standard reduction potential table?
Determine the overall reaction and its standard cell potential at 25 C for this reaction. Is the reaction spontaneous at standard conditions? Cu(s)|Cu2+(aq)Au3+(aq)|Au(s)
Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaueous under each set of conditions at 293.15 K. (a) Hg(l)+S2(aq,0.10M)+2Ag+(aq,0.25M)2Ag(s)+HgS(s) (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half—cell consisting of a nickel electrode in 025 M nickel(l) nitrate solution. (c) The cell made of a half-cell in which 1.0 M aqueous bromide is oxidized to 0.11 M bromine ion and a half-cell in which aluminum ion at 0.023 M is reduced to aluminum metal. Assume the standard reduction potential for Br2(l) is the same as that of Br2(aq).