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22 Cards in this Set

  • Front
  • Back
What should you note about a galvanic cell?
(1) the cell potential must be greater than zero.
(2) cell potential is equal to the cathode potentail minus the anode potential when they are written as reductions.
(3) reduction - the gain of electrons - occurs at the cathode.
(4) oxidation - the loss of electrons - occurs at the anode.
For galvanic cell, the electrode with the highest reduction potential will be the (cathode/anode)?
When an electrochemical cell operates spontaneously, it is called a _______.
galvanic cell.
For voltaic cell, if the cell potential is positive, G is (less/greater) than zero.
- Less than zero, by the relationship G=-nFE;
- and therefore spontaneous
In a voltaic cell, the electrons always flow from the (anode/cathode) to the (anode/cathode).
- anode to cathode.
- electrons are loss at the anode; and gained at the cathode.
For a voltaic cell, what happens when the flow of electrons stop?
(1) the cell potential is zero.
(2) the system is at equilibrium (recall the reationship G=-nFE).
(T/F) For a voltaic cell at equilibrium, the concentration of no reactant or product goes to zero.
(T/F) Electrochemical reactions are spontaneous.
False; they are not spontaneous. They can be driven to completion by passing an electric current through the solution (process is called electrolysis and the cell is called an electrolytic cell).
How is an electrolytic cell different from a galvanic cell?
In an electrolytic cell, the anode is positively charged and the cathode is positively charged; which is opposite to that of the galvanic cell.
(T/F) Reduction occurs at the cathode; and oxidation occurs at the anode for both the galvanic and electrolytic cell.
What is positively and negatively charged in the electrolytic cell?
cathode = negatiuve
anode = positive
What is positively and negatively charged in the galvanic cell?
cathode = positive
anode = negative
What is the faraday constant?
- magnitude of the charge of one mole of electrons.
- used in equation G=-nFE and Nernst equation.
What are exsamples of strong electrolytes?
NaCl, KCl, HCl, HBr, and HI.
What are example of weak electrolytes?
water, HF< acetic acid, benzoic acid, and ammonia.
What is an electrolyte?
a substance that ionizes to yield an electrically conducting solution;
- a strong electrolyte is one that ionizes completely or nearly completely, and a weak electrolyte doesn't ionize very much at all.
What is the reationship between charge, amperes and time?
Charge is equal to current in Amps times time in seconds.
Is pure water an electrolyte?
No; it will not conduct electricity.
What charge does a carbonate ion have?
-2 charge;
If something is precipitated, what should you think if you see a bunch of reactions?
look for the solid!
(T/F) The hydroxides of all Group I and II metals are strong bases.
What are the most common strong acids?
sulfuric acid (H2SO4),
nitric acid (HNO3),
hydroclhloric acid (HCl),
Hydrobromic acid (HBr),
Hydroiodic acid (HI),
Chloric Acid (HClO3),
perchloric acid (HClO4)