Chapter 17: Electrochemistry. Review of Redox Reactions Galvanic Cells: Using spontaneous redox reactions to generate electrical energy. Galvanic Cells Cell potential D G and work Cell potential and concentration Applications: Batteries, fuel cells, corrosion
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Balance the following redox reactions
using the half reaction method.
If a standard Cu|Cu2+ electrode is
connected to a standard Al|Al3+
electrode, what reaction occurs? What
is °cell? Sketch the cell, label the
cathode and anode, show the direction
of electron flow, and give the line
notation for the cell.
Consider the following species under
Ce4+, Ce3+, Fe2+, Fe3+, Fe, Mg, Mg2+, Ni2+, Sn
Select an oxidizing agent to oxidize Cl-
to Cl2 without oxidizing Br- to Br2.
Calculate the maximum work available
from 25.0 g of aluminum in the
following galvanic cell for which the emf
is 1.15 V. Note that O2 is reduced to
H2O in this reaction.
Calculate the cell potential for the
following Galvanic cell at 25°C.
Find the potential of a
Ag+(1.0x10-7M)|Ag(s) electrode at 25°C.
Calculate the equilibrium constant for
the following reaction at 25°C.
Ag+(aq) + Fe2+(aq) Ag(s) + Fe3+(aq)
A concentration cell is made up of two
Ag/Ag+ half cells. In the first half cell,
[Ag+] = 0.010 M. In the second half
cell, [Ag+] = 4.0 x 10-4 M. What is the
cell potential? Which half cell functions
as the anode?
Predict the products and calculate the
minimum voltage required for the
electrolysis of the following substances
using platinum electrodes.
Write the net ionic equation for the
reaction you expect to occur when the
electrolysis of NiSO4(aq) is conducted
using a nickel anode and an iron
How many grams of silver are deposited
at a platinum cathode in the
electrolysis of an aqueous solution of
AgNO3 by 1.73A of electric current in
How long will it take to produce 10.0 g
of bismuth (Bi) by the electrolysis of a
BiO+ solution using a current of 25.0 A?