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Date Lecture/Activities Pg#
93. 05/19/15 Electrochemistry 154
Objective:
I will record lecture notes to identify how redox reaction are used to generate energy in voltaic and electrolytic cells.
Chemcatalyst:
1.Given reaction rate data for: F2(g) + 2ClO2(g) --> 2FClO2(g)
Experiment [F2](M) [ClO2](M) Initial Rate (M/s)
1 0.10 0.010 1.2 x 10-3
2 0.10 0.040 4.8 x 10-3
3 0.20 0.010 2.4 x 10-3
A. Determine the order of each reactant and the overall reaction order.
(Hint: [ ] = k x=order)
x
A measure of the amount of current that can be generated from a voltaic cell to do work
* Electric charge can flow between two points only when a difference in electric potential energy exists between two points.
*Electromotive forces push the electrons generated at the anode to the cathode
*Cell Potential: force produced by the difference in potential energy between the two electrodes (measured in volts)
*Voltage: determined by comparing the difference in the tendency of the two electrode materials to accept electrons
-the greater the difference, the greater the PE difference
between the two electrodes & the larger the voltage
consist of a small sheet of platinum immersed in a hydrochloric acid solution that has a hydrogen-ion concentration of 1M. Hydrogen gas at a pressure of 1 atm is bubbled in and the temperature is maintained at 25 degrees celsius
Oxidation
Reduction
The study of the redox processes by which chemical energy is converted to electrical energy and vice versa
Involve the transfer of electrons from the oxidized species to the reduced species.
Oxidation - losing electrons (anode)
Reduction - gaining electrons (cathode)
Half Cells: parts of electrochemical cell that separate the oxidation and reduction reactions
Use the values of the known Standard Reduction Potentials to calculate the overall Cell Potential
oxidation
reduction
- -
2
-
2+
The following reduction half-reaction s represent the half-cells of a voltaic cell.
I (s) + 2e 2I (aq)
Fe (aq) + 2e Fe (s)
Determine the overall cell reaction and the standard cell potential. Describe the cell using cell notation.
* The half reaction with the lowest reduction potential will be the oxidation
* (+) values of cell potential: spontaneous
* (-) values of cell potential: not spontaneous