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

6) Calculate the potential of a cell, Eºcell, made with a standard bromine electrode as the anode and a standard chlorine electrode as the cathode. Write the shorthand cell notation.

A certain half-reaction has a standard reduction potential Ered = -1.01 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used…

4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.

A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative

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Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode.   MnO4-  +     H+    +      Ce3+     ->         Ce4+     +     Mn2+    +      H2O

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