# chemistry

A voltaic cell is contructed in which a copper wire is placed in a 1.0 M Cu(NO3)2 solution and a strip of gold i placed in a 1.0 M AuNO3 solution. The measured potential of the cell is found to be 1.36V and the copper electrode is negative. The Ered for the Cu2+/Cu half- cell is +0.34

a) Since the copper electrode is negative, oxidation takes place at the copper electrode. Write the oxidation half-reaction for the Cu2+/Cu half-cell and indicate its standard oxidation potential, Eox

b)Write the half-reaction for the Au2+/Au half-cell.

c) write the overall balanced oxidation-reduction and indicate the standard cell potential Ecell

d) Calculate the standard reduction potential Ered for the Au2+/Au half-cell

1. 0
2. 16
1. a)
Cu ==> Cu^+2 + 2e and Eo = -0.34

b)
Au^+2 + 2e ==> Au

c)
Add a and b to obtain c and Ecell = 1.36 v

d)
If (a) is -0.34 v and the total cell (part c) is 1.36 v, what must (b) be; i.e.,
-0.34 + ? = 1.36
Note: There seems to be a discrepancy between the problem statement about AuNO3 and the question in part b.

posted by DrBob222

## Similar Questions

1. ### chem 2

Consider a chromium-silver voltaic cell that is constructed such that one half-cell consists of the chromium, Cr, electrode immersed in a Cr(NO3)3 solution, and the other half-cell consists of the silver, Ag, electrode immersed in
2. ### Chemistry

Consider a chromium-silver voltaic cell that is constructed such that one half-cell consists of the chromium, Cr, electrode immersed in a Cr(NO3)3 solution, and the other half-cell consists of the silver, Ag, electrode immersed in
3. ### Chemistry

Consider the voltaic cell illustrated in the figure, which is based on the cell reaction: Zn(s)+Cu^2+(aq) -> Zn^2+(aq)+Cu(s) Under standard conditions, what is the maximum electrical work, in joules, that the cell can accomplish
4. ### Chemistry

Consider the voltaic cell illustrated in the figure, which is based on the cell reaction: Zn(s)+Cu^2+(aq) -> Zn^2+(aq)+Cu(s) Under standard conditions, what is the maximum electrical work, in joules, that the cell can accomplish
5. ### chem

Explain, in terms of electrical energy, how the operation of a voltaic cell differs from the operation of an electrolytic cell used in the Hall process. Include both the voltaic cell and the electrolytic cell in your answer. Would
6. ### apchemistry

Hi Please double check me: I had to state whether the process forms a voltaic or eletrolytic cell: YOu plug in your MP3 player to charge the nickel-cadmium battery (I said electrolytic)??? The radio plays in your car even though
7. ### Chemistiy

Check if im right please. a. oxidation occurs at my anode ____ ** Voltaic Cell b. You can use standard reduction potential table to calculate how much voltage it takes to operate me____ **Both voltaic cell and electrolytic cell
8. ### Chemistry again

Two voltaic cells are to be joined so that one will run the other as an electrolytic cell. In the first cell, one half-cell has Au foil in 1.00M Au(NO3)3, and the other half-cell has a Cr bar in 1.00M Cr(NO3)3. In the second cell,
9. ### Chemistry

One half-cell in a voltaic cell is constructed from a silver wire electrode in a .25 M solution of AgNO3 . The other half-cell consists of a zinc electrode in a .001 M solution of Zn(NO3)2. Calculate the cell potential I have no
10. ### chemistry (electrochemistry)

1) For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 1.50 M)|Ag(s) write the net cell equation. Calculate the following values using standard potentials as needed. Eo cell and dGo for each

More Similar Questions