Electrochemical Cells
The tendency of oxidation-reduction reactions is to proceed to an equilibrium state. These reactions occurring in electrochemical cells provide another way for us to express the driving force in chemical reactions. When reagents that accept or donate electrons are arranged so that the electrons can enter or leave the reaction through a metallic conductor, an electrochemical cell is established. A half-cell contains a metal in contact with a solution of its salt. Each metal will develop a different electrical potential based on its electron configuration. The standard reduction potential listed in various references is the voltage that a half-cell develops when combined with a hydrogen half-cell. First, construct a simple chemical battery and determine from the standard reduction potentials what the output of the battery will be (if a voltmeter is available the actual and theoretical voltages can be compared). Second, construct an electrolysis cell and demonstrate how hydrogen and oxygen can be produced from the electrolysis of water.
Kit Includes:
- Cupric Sulfate, 0.5M Solution - 500 ml x 2 Bottles
- Bromothymol Blue, 0.04% Solution - 25 ml x 1 Bottle
- Sodium Sulfate, 1M Solution - 500 ml x 8 Bottles
- Copper Metal Strips - 15 pcs
- Magnesium Metal Strips 5 Inch UN1869 - 15 pcs
- Dialysis Tubing Strips 6 Inch - 15 pcs
Materials needed but not supplied:
- (# 6131-4) Beaker 250 ml - 30 pcs
- (# 6135-3) Test Tube 13 x 100 mm - 30 pcs
- (# 1931-2) Flashlight Bulb 1.5 v - 15 pcs
- (# 1602-31) Wire Leads with Alligator Clips - 15 pairs
- 9V Batteries - 15 pcs
Optional materials:
- (# 1743-25) Voltmeters - 15 pcs
Please note that the pictures below may show items not included in this kit, the pictures are there to show kit functionality. Please refer to the product details above for more information on the contents of this kit.
DOT: Small quantity exemption 173.4. This package conforms to 49 CFR 173.4 for domestic highway or rail transport only
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