(a) How many moles of mercury will be produced by electrolysing 1.0 M Hg(N03)2 solution with a current of 2.00 A for 3 hours?[Hg(N03)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(N03)2 solution with a current of 2.00 A for 3 hours?[Hg(N03)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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.50QE
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(a) How many moles of mercury will be produced by electrolysing 1.0 M Hg(N03)2 solution with a current of 2.00 A for 3 hours?
[Hg(N03)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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