(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)

The quantity of charge passed is calculated as follows, Q=I×t Where,…

Answered: (a) How many moles of mercury will be…

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...

See similar textbooks

Related questions

Concept explainers

Question

(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;E_Ni2+/Ni= – 0.25 V,E_Al3+/Al= – 1.66 V)

Expert Solution

Step by step

Solved in 6 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions