1.) A sodium sulfate solution was electrolyzed using inert Pt electrodes. The cathode reaction was 2H2O + H2+2OH^-. If a current of 3.0 amp was used for 30 min, what weight of H2O gas would be produced?

1.) A sodium sulfate solution was electrolyzed using inert Pt electrodes. The cathode reaction was 2H2O + H2+2OH^-. If a current of 3.0 amp was used for 30 min, what weight of H2O gas would be produced?

2.) What volume of H2 gas at STP would be produced during the passage of 30,000 Coul in the electrolysis of H2O?

3.) Give the notation for the cell that utilizes the reaction: 

(a) Cl2 (g)+ 2 I^-(aq) to 2 Cl^-(aq)+I2(s), 

(b) what is the E^o for the cell?

(c) which electrode is the cathode?

4.) The standard electrode potential fornthe Fe^2+ to Fe^(3+) + e - half reaction is  -0.770V.

(a) Using the Nernst equation [E=E^o - (0.059/n) log [Oxid]/[Red]]. Calculate the voltage of this half cell when the [Fe^3+] is 1.0 x 10^-3 and [Fe^2+] is 1.0 x 10 ^ -1.

(b) Calculate the approximate equilibrium constant (K) for the half reaction.