Fe(s) Fe²+ (aq) || MnO4 (aq), Mn²+ (aq)| Pt(s) | Write the half reactions: Oxidation: Reduction: Net standard potential, E (in volts): Is the cell Galvanic or Electrolytic cell?: Which is the Anode: Cathode: Which electrode increases in mass during the reaction: Write the balance chemical equation for this cell (in acidic condition):

a) Balance the following reactions.  b) Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions.  c) Identify the reactions with K > 1 among the following redox reactions.  d) Write the line representations for the Galvanic cells, indicating the anode and cathode. Cl2 +  Br- -->  Cl-   +    Br2 MnO4- +  H+  +  Ce3+  --> Ce4+  +  Mn2+  +  H2O Pb2+ -->Pb  +  Pb4+ NO3- +  H+ +  Zn  -->  Zn2+   +  NO2  +  H2O

In the given electrochemical cell, what is the cathode half-reaction? Zn(s) | Zn2+(aq) || Fe3+(aq), Fe2+(aq) | Pt(s)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)

What mass of material will be deposited at the cathode when a current of 10.5 A is applied for 2.0 hours to the following cell: Cr(s) | Cr² (aq) || Al*(aq) | Al(s)

Two half-reactions are shown with their standard cell potentials. If a galvanic cell is constructed using them, which electrode would be the anode, and what would the cell potential be? Cd2* (aq) + 2e – Cd(s); E=-0.40 V Cr3+ (aq) + 3e → Cr(s); E=-0.74 V Oa. Cadmium, -0.34 V Ob. None of the other options Oc. Cadmium, -1.14 V Od. Chromium, -1.14 V Oe. Chromium, 0.34 V

What is the maximum amount of work that could be done by the following electrochemical cell? Sn(s))SnSO4(aq)||Au(NO;);(aq)|Pt(s)

calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C Fe(s) | Fe3+ (aq, 0.0011M) || Fe3+(aq, 2.33M) | Fe(s)

A galvanic cell is powered by the following redox reaction: 2+ 3+ O,(g) + 4H'(aq) + 4 Fe´'(aq) 2 H20(1) + 4 Fe"(aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E° = [v Round your answer to 2 decimal places.

The following figure represents an electrochemical cell at 25.00C with aqueous solutions that behave ideally: (a) Represent the electrochemical cell using cell notation, by taking into account that concentrations of the ZnSO4 and CuSO4 solutions are 0.25 M and 0.35 M, respectively. (b) Calculate the standard potential of the cell, E0cell. (c) Calculate the potential of the cell, Ecell. (d)Calculate DG0 (e)Calculate DG (f)Calculate the equilibrium constant, K.