A zinc-copper battery is constructed at follows at 25°C: Zn /  Zn2+(0.10M) // Cu2+(2.50 M) / Cu The mass of each electrode is 200. g.a.  Calculate the cell potential when this battery is first connected.b.  Calculate the cell potential after 10.0 A of current has flowed for 10.0 h. (Assume each half-cell contains 1.00 L of solution.)c.  Calculate the mass of each electrode after 10.0 h.d.  How long can this battery deliver a current of 10.0 A before it goes dead?

20). Calculate the cell voltage for the electrochemical cell below. Assume standard conditions. Note: Sulfate is not in any of the solutions. Ni(s) /Ni2* (aq, 1.0 M) //Pb²* (aq, 1.0 M) /Pb(s) a. +0.106 V b. +1.935 V C. +0.124 V d. +0.606 V e. None of the above

Using a table of standard electrode potentials, decide which of the following statements is completely true. Multiple Choice cu2" can oxidize H2, and Fe can reduce Mn2". H* can oxidize Fe. and NI can reduce Br2. Ni2" can oxidize Cu?", and Fe2* can reduce H". Fe?" can oxidize H2, and Fe2“ can reduce Au3". Br2 can oxidize NI, and H2 can reduce Mn*.

A.  From the reaction as shown below, calculate the Standard Cell Potential of a Galvanic Cell that uses the half-reactions shown below.                              Cr3+    +    3e-    ------->     Cr               Eo = -0.73 V                             Al3+    +    3e-    ------->     Al              Eo = -1.66 V B. A galvanic cell is made using 0.25M ZnSO4 and an unknown amount of CuSO4. The cell potential is 105V at 50oC. What is the concentration of CuSO4 in the cathode compartment?         Zn(s)   +   Cu(aq)2+   ------->   Zn(aq)2+   +   Cu(s)          Eo = 1.10 V Use:E = Eo - (RT/nF) + lnQ

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