Wednesday, March 21, 2007
Figuring out E* at different pH's of water
There was one exam problem in which it asked you to calculate the E* of 2H+ + 2e- --> H20 at pH of 5. Will this type of problem be on the test, and if so what is the basic way to solve this problem.
Wednesday, March 7, 2007
Workshop post
sorry for the late post but here it is:
Oxidizing agent is in Cathode. Reducing agent is in Anode.
Negative ions (such as NO3-) leave salt bridge to the ANODE to prevent build up of positive charge (which would stop the system)
Positive ions (such as K+) leave salt bridge to the Cathode to prevent build up of negative charge (which would stop the system)
Electrons flow from anode to cathode.
finally (i know its been saiid but its important): REDUCTION POTENTIAL IS THE ABILITY OF SOMETHING TO BE REDUCED!!!!!!!!! HIGHER REDUCTION POTENTIAL WILL OXIDIZE ANYTHING WITH A LOWER REDUCTION POTENTIAL. IT IS A REALLY GOOD OXIDIZING AGENT. (and vice versa for a high oxidation potential).
Oxidizing agent is in Cathode. Reducing agent is in Anode.
Negative ions (such as NO3-) leave salt bridge to the ANODE to prevent build up of positive charge (which would stop the system)
Positive ions (such as K+) leave salt bridge to the Cathode to prevent build up of negative charge (which would stop the system)
Electrons flow from anode to cathode.
finally (i know its been saiid but its important): REDUCTION POTENTIAL IS THE ABILITY OF SOMETHING TO BE REDUCED!!!!!!!!! HIGHER REDUCTION POTENTIAL WILL OXIDIZE ANYTHING WITH A LOWER REDUCTION POTENTIAL. IT IS A REALLY GOOD OXIDIZING AGENT. (and vice versa for a high oxidation potential).
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