# Chemistry

posted by .

Using your experimental data, calculate E0cell. Standard voltaic cells contain 1M solutions, but we used 0.10M solutions in all of our half cells. Use the Nernst equation to calculate the standard cell potential (E0cell) from your measured Ecell and Qrxn.

Data:
Nernst Equation: Ecell=E0cell -RT/nF ln Q

Questions:

1. I am not sure if i did the E0cell right equation, I switched the Ecell to get the E0cell..and "n" is equal to 2 moles being transfer?

I calculated:
Measured Ecell = 0.445V
Overall rxn = Cu(s)+Pb2(aq) ~ CU2+(aq) + Pb(s)
N= 2moles??

Re-arrange the equation:
E0cell = Ecell - RT/nF ln Q
E0cell = 0.445V -(8.314 j/k*mol *298K)/(2 moles * 96500 c/mole e-) ln (0.10)
= -2.30

2. Overall reaction:
3Pb(s) + 2Al 3+ (aq) ~ 3Pb2+(aq) = 2Al(s)
Measured Ecell(V) = 0.086V
N= 6moles?? (3*2 moles)

0.086V- (8.314 j/k*mol * 298K)/ (6moles * 96500 C/mole e- ) ln (0.10/0.10^6) = 0.94??

## Similar Questions

1. ### Chemistry

1) Assume that the reference half-cell is changed to a standard mercury-mercury (II) half-cell. a) What would be the reduction potential of a standard chlorine half-cell. c) What would be the cell potential of a standard chlorine-nickel …
2. ### 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, …
3. ### chemistry

A voltaic cell at 25oC consists of Mn/Mn2+ and Cd/Cd2+ half-cells with the initial concentrations [Mn2+] = 0.100 M and [Cd2+] = 0.0100 M. Use the Nernst equation to calculate E for this cell. Cd+2(aq) + 2e- = Cd(s) . . . . . . Eo = …
4. ### 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 …
5. ### electrochemistry

Calculate the cell potential of voltaic cells that contain the following pairs of half-cells. a)A half-cell containing both HgCl2 and Hg2Cl2; lead in a solution of Pb2+ ions.
6. ### chemistry

Calculate the cell potential of voltaic cells that contain the following pairs of half-cells. a)A half-cell containing both HgCl2 and Hg2Cl2; lead in a solution of Pb2+ ions.
7. ### chemistry

1. If half cell A has a standard reduction potential of E= -1.10 V and half cell B has a standard reduction potential of E= 0.65 V, which half-cell is the anode?
8. ### chemistry

Consider two cells, the first with Al and Ag electrodes, and the second with Zn and Ni electrodes, each in appropriate 1.00 M solutions of their ions. a) If connected as voltaic cells in series, which two metals are plated, and what …
9. ### Chemistry

How to calculate Q in Nernst Equations, we used 0.10M solutions in all of our half cells. Nernst equation: Ecell = E0cell - RT/nF ln Q Overall reactions: Cu(s) + Pb2+(aq) ~ Cu2+(aq) + Pb(s) and 3Pb(s) + 2Al3+ ~ 3Pb2+ 2Al(s) Thank you!
10. ### Chemistry

The cell diagram for the lead-acid cell that is used in automobile and truck batteries is Pb(s) l PbSO4 (s) l H2SO4 (aq) l PbO2(s), PbSO4(s) l Pb (s) where the comma between PbO2 (s) and PbSO4 (s) denotes a heterogeneous mixture of …

More Similar Questions