Hi. Can someone please explain to me how to do the following question? I'm quite confused about how to do these. See attachment for better notation representation.

Consider the following reaction at 25 degrees C, [Al3+] = 2.0 M and [Zn2+] = 1.0M

2 Al (s) + 3 Zn2+ (aq) -> 3 Zn (s) + 2 Al3+ (aq)

a) Predict if the cell potential, Ecell > Eocell or Ecell < Eocell. Explain why.
(I don't know how to determine this. Actually, I'm not even certain what the difference is between Ecell and Eocell. Please explain.)

b) Calculate Eocell given the half-reduction potentials.

Zn2+ (aq) + 2 e- -> Zn (s) Eo = -0.76 V
Al3+ (aq) + 3 e- -> Al (s) Eo = -1.66 V

I think the Eocell = +1.66 - 0.76 = +0.9 V
Is that right?

c) How many electrons are transferred in the reaction?

Is the answer 6 e-?

d) Calculate Ecell for the reaction using the Nernst equation.

I really don't know how to do this one. I know that the Nernst equation is
Ecell = Eocell (-RT/nF) ln Q, but I'm not sure what Q is or what Temp to apply here.

This solution contains stepwise explanations that differentiates Ecell and Eocell, as well as calculates the Eocell for the half-reduction potentials and how many electrons are transferred in the reaction. In addition, the Nernst equation is explained and used to calculate Ecell.

Standard potentials are measured against the standard hydrogen electrode (S.H.E.). Because it is not always convenient to use a S.H.E., often other reference electrodes are used. The saturated calomel electrode (S.C.E.) is one commonly used reference electrode, with a potential of 0.242 V versus the S.H.E. Using a table of stand

Consider the electrochemical cell:
Pt|Cr2+(0.2752 M), Cr3+(1.705 M)||Co2+(0.2008 M)|Co
a. What is the cellpotential (hint: you can solve the problem by half-reactions or by the over-all reaction, both will give you the same answer so you can double check yourself)?
b. Is the cell galvanic or electrolytic (must show math i

Please see the attached file for the fully formatted problems.
Question 1.
In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods: the half-reactio

Hello, I am working on a lab and trying to verify my results with what the "expected" value should be. Please help me by answering the following question:
Use standard electrode potentials to calculate the voltage of a cell using:
a) Zn/Zn 2+ and Pb/Pb 2+ half cells.
b) Zn/Zn 2+ and Cu/Cu 2+ half cells
c) Cu/Cu 2+ a

Describe an electrochemical cell that would determine the solubility product constant at equilibrium for Chronium (III) hydroxide, then calculate the solubility product constant.
Balance these reduction potential half equations first:
Ox. Cr+3(aq) + 3e => Cr(s) -0.74v
Red. Cr(OH)3(s)

a). Give the cell diagram notation of the electrochemical cell that could be used to determine experimentally the dissociation constant (Kw) of water. The standard reduction potential for
O2 + 2H2O + 4 e-------> 4OH- is + 0.40V
For other half-reactions, use a textbook. Calculate E for this cell.
b). Use yo

Given the following standard electrode reductionpotentials,
ClO3- + 2H2O <- -> ClO- + 4OH- E° = +0.50V
ClO- + H2O + 2e- <- -> Cl- + 2OH- E° = +0.89V
Predict whether or not CLO- will disproportionate in alkaline solution to give Cl- and ClO3- according to the following reaction:
3C

1. Using data in Appendix E, calculate the standard emf for each of the following reactions:
(a) H2(g) + F2(g) → 2 H+(aq) + 2 F-(aq)
(b) Cu2+(aq) + Ca(s) → Cu(s) + Ca2+(aq)
(c) 3 Fe2+(aq) → Fe(s) + 2 Fe3+(aq)
(d) 2 ClO3-(aq) + 10 Br-(aq) + 12 H+(aq) → Cl2(g) + 5 Br2(l) + 6 H2O(l)
2. Using the standard reduction po

Give brief explanations (3 or 4 lines) for the following:
a). Silver is oxidized by nitric acid, but gold is resistant to oxidation by nitric acid.
b). Aluminium does not corrode readily in moist air, but iron does.
c). You should not replace a section of galvanized iron pipe with copper pipe when doing plumbing repairs.
d