(a) How many moles of mercury will be produced by electrolysing 1.0 M Hg(NO3)2 solution with a current of 2.00 A for 3 hours?[Hg(NO3)2 = 200.6 g mol-1](b) A voltaic cell is set up at 25 °C with the following half-cells:Al3+(0.001 M) and Ni2+(0.50 M)Write an equation for the reaction that occurs when the cell generates an electric current and determine the cell potential.(Given; ENi2+/Ni = – 0.25 V, EAl3+/Al = – 1.66 V)
(a) How many moles of mercury will be produced by electrolysing 1.0 M Hg(NO3)2 solution with a current of 2.00 A for 3 hours?[Hg(NO3)2 = 200.6 g mol-1](b) A voltaic cell is set up at 25 °C with the following half-cells:Al3+(0.001 M) and Ni2+(0.50 M)Write an equation for the reaction that occurs when the cell generates an electric current and determine the cell potential.(Given; ENi2+/Ni = – 0.25 V, EAl3+/Al = – 1.66 V)
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter21: The Chemistry Of The Main Group Elements
Section: Chapter Questions
Problem 108SCQ
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(a) How many moles of mercury will be produced by electrolysing 1.0 M Hg(NO3)2 solution with a current of 2.00 A for 3 hours?
[Hg(NO3)2 = 200.6 g mol-1]
(b) A voltaic cell is set up at 25 °C with the following half-cells:
Al3+(0.001 M) and Ni2+(0.50 M)
Write an equation for the reaction that occurs when the cell generates an
(Given; ENi2+/Ni = – 0.25 V, EAl3+/Al = – 1.66 V)
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