In an electrolytic cell, a current of 0.250 ampere is passed through a solution of a chloride of iron, producing solid Fe and chloride gas (Cl2).
a. Write the equation for the half-reaction that occurs at the anode.
b. When the cell operates for 2.00 hours, 0.521 grams of iron is deposited at one electrode. Determine the formula of the chloride of iron in the original solution.
c. Write the balanced equation for the overall reaction that occurs in the cell.
d. How many liters of chlorine gas, measured at 25 degreeC and 750mmHg, are produced when the cell operates as described in part B?
e. Calculate the current that would produce chlorine gas from the solution at a rate of 3.00 grams per hour.
Problem #2
A galvanic cell (electrochemical cell) is made from zinc and iron (from Fe2+ to Fe0 or visa versa).
a. Determine the overall chemical reaction and Ecell0
b. Sketch the cell including direction of flow of electrons, anode (half-cell rxn, material of anode,and solution at anode), cathode(same as anode).
c. Calculate deltaG0 and K for this reaction at 25 degreeC.
d. Calculate Ecell at 25degreeC when [Zn2+]= 0.10M and [Fe2+] = 1.0E-5M.