a. Under standard conditions at 25C, Zn(s) reacts with Co2+ (aq) to produce Co(s)
i. Write the balanced equation for the oxidation half reaction.
ii. Write the balanced net ionic equation for the overall reaction.
iii. Calculate the standard potential, E, for the overall reaction at 25C.
b. At 25C, H2O2 decomposes according to the following equation.
2H2O2(aq) => 2H2O (l) + O2(g) .55V
i. Determine the value of the standard free energy change, Delta G, for the reaction at 25C.
ii. Determine the value of equilibrium constant, Keq, for the reaction at 25C.
iii. The standard reduction potential, E , for the half reaction O2(g) + 4H+(aq) + 4e- => 2H2O(l) has a value of 1.23V. Using this information in addition to the information given above, determine the value of the standard reduction potential, E, for the half reaction below.
O2(g) + 2H+(aq) +2e- => H2O2(aq)
c. In an electrolytic cell, Cu(s) is produced by the electrolysis of CuSO4(aq). Calculate the maximum mass of Cu(s) that can be deposited for a direct current of 100 amperes passed through 5.00L of 2.00M CuSO4(aq) for a period for 1 hour.
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