Chemistry

I'm having trouble with the following question, any help would be greatly appreciated.

A voltaic cell consists of a Zn/Zn^2+ half-cell and a Ni/Ni^2+ half-cell at 25 C . The initial concentrations of Ni^2+ and Zn^2+ are 1.30 M and 0.100 M , respectively.

What is the cell potential when the concentration of Ni^2+ has fallen to 0.500 M?

What is the concentrations of Ni^2+ when the cell potential falls to 0.45 M?

What is the concentration of Zn^2+ when the cell potential falls to 0.45 M?

  1. 👍
  2. 👎
  3. 👁
  1. I haven't tried to work on this problem at all because I don't understand how Ni2+ ion can start at 0.100M, use some of it and END UP FALLING to 0.500M. It appears to me that Ni2+ can become smaller but not larger.

    1. 👍
    2. 👎
  2. The second part of this question does not make sense cell potential has to be in V not M...M is for concentration

    1. 👍
    2. 👎
  3. I got the correct answer by making a simple Initial/Final chart. the initial [Ni^2+] = 1.30, the final [Ni^2+] = 0.500. The change is 0.80 M. This means you would add 0.80 to the initial [Zn^2+] (which is .100 M) and you would get a final [Zn^2+] of 0.90 M.
    The next step is to find the new Q which is [Zn^2+]/[Ni^2+] = (0.90)/(0.500). Plug this in the Nernst equation and you will find the cell potential.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    A voltaic cell that uses the reaction Tl3+(aq) + 2 Cr2+(s) ¨ Tl+(aq) + 2 Cr3+(aq) has a measured standard cell potential of +1.19 V. determine E‹red for the reduction of Tl3+(aq) to Tl+(aq).

  2. chemistry

    A voltaic cell consists of a standard hydrogen electrode in one half-cell and a Cu/Cu2+ half-cell. Calculate [Cu2+] when E cell is 0.22 V.

  3. chemistry

    Calculate the pH for the hydrogen half-cell of the following voltaic cell if the observed cell voltage is 1.00 V. Mn|Mn2+(1.00 M)||H+(pH =?), H2(1.00 atm)|Pt

  4. chemistry 2

    A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb2+ half-cell. Measurement shows that thesilver electrode is positive. -Write balanced half-reactions and the overall spontaneous reaction.

  1. CHEMISTRY

    A voltaic cell is constructed that uses the following reaction and operates at 298 K: 2 Al(s) + 3 Mn^2+(aq) 2 Al^3+(aq) + 3 Mn(s). What is the potential, E, of this cell when [Mn^2+] = 0.10 M and [Al^3+] = 1.5 M?

  2. 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

  3. Chemistry

    A voltaic cell utilizes the following reaction and operates at 298K 3Ce{4+}(aq)+Cr(s)--->3Ce{3+}(aq)+Cr{3+}(aq) {}=Charge What is the EMF of this cell under standard conditions? What is emf of cell when [Ce{4+}]=2.1M,

  4. Chemistry

    12. In a calorimeter, 10 g of ice absorbs heat with an enthalpy of fusion of 334 J/g. What is the heat absorbed? q = mCHf I am having a lot of trouble on this type of problem in chem. Help and an explanation would be greatly

  1. Chem 2

    A voltaic cell consists of an Al/Al3+ half-cell and a Cd/Cd2+ half-cell. Calculate {Al3+} when {Cd2+} = 0.401 M and Ecell = 1.299 V.Use reduction potential values of Al3+ = -1.66 V and for Cd2+ = -0.40 V.

  2. 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

  3. Chemistry

    A voltaic cell utilizes the following reaction: 2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq). What is the emf for this cell when [Fe3+]= 3.70M , PH2= 0.95atm , [Fe2+]= 7.0×10−4M , and the pH in both compartments is 4.05? Express your

  4. College Chemistry

    For the reaction that occurs in the voltaic cell Fe(s)|Fe2+(aq)||Cr3+(aq),Cr2+(aq)|Pt(s) use data from Appendix D in the textbook to answer the following questions: a)Determine the equation for the cell reaction b)Determine E0

You can view more similar questions or ask a new question.