A galvanic cell at a temperature of 42°C is powered by the following redox reaction:
3CU2+(aq) + 2Al(s) > 3Cu(s) + 2Al3+(aq)
Suppose the cell is prepared with 3.43 M Cu2+n one half-cell and 1.63 M Al3+in the other.
(A) Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

1.99V

Explanation:

Balanced redox reaction equation:

3CU2+(aq) + 2Al(s) > 3Cu(s) + 2Al3+(aq)

E°cell= E°cathode- E°anode

E°cell= 0.34-(-1.66)

E°cell= 2.0V

From Nernst equation:

E= E°cell - 0.0592/n logQ

E= 2.0 - 0.0592/6 log [3.43]/[1.63]

E= 2.0- 0.0032

E= 1.99V

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

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~ trueboss72