2. A galvanic cell is constructed that has a zinc anode immersed in a Zn(NO3)2 solution and a platinum cathode immersed in an NaCl solution equilibrated with Cl2 (g) at 1 atm and 25oC. A salt bridge connects the two half-cells. a. Write a balanced equation for the cell reaction. b. A steady current of 0.800 A is observed to flow for a period of 25.0 minutes. How much charge passes through the circuit during this time? How many moles of electron is this charge equivalent to? c. Calculate the change in mass of the zinc electrode. d. Calculate the volume of gaseous chlorine generated or consumed as a result of the reaction.

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