Question

In an electrochemical cell the reaction occurs: Zn (s) + Fe+ 3 (aq) -> Zn+ 2 (aq) + Fe+ 2 (aq). The reduction potentials are: Fe+ 3 (ac) + e- -> Fe+ 2 (ac) E ° = 0.771 V Zn+ 2 (ac) + 2e- -> Zn (s) E ° = -0.763 V a) Write down the half-reaction that occurs at the anode and indicate whether oxidation or reduction is occurring. b) Write down the half-reaction that occurs at the cathode and indicate whether oxidation or reduction is occurring. c) Balance the redox reaction. d) Calculate the potential of the cell if [Zn+ 2] = 0.93 M, [Fe+ 2] = 0.10M and [Fe+ 3] = 0.81 M at 25 ° C. e) Write the notation (shorthand notation) for the electrochemical cell.

          In an electrochemical cell the reaction occurs: Zn (s) +
Fe+ 3 (aq) -> Zn+ 2 (aq) + Fe+
2 (aq). The reduction potentials are:  
 Fe+ 3 (ac) + e- -> Fe+ 2 (ac)
  E ° = 0.771 V            
Zn+ 2 (ac) + 2e- -> Zn (s)   E ° = -0.763 V
               
a) Write down the half-reaction that occurs at the anode and
indicate whether oxidation or reduction is occurring. 
b) Write down the half-reaction that occurs at the cathode and
indicate whether oxidation or reduction is occurring. 
c) Balance the redox reaction. 
d) Calculate the potential of the cell if [Zn+ 2] =
0.93 M, [Fe+ 2] = 0.10M and [Fe+ 3] = 0.81 M
at 25 ° C. 
e) Write the notation (shorthand notation) for the
electrochemical cell.

Added by Samantha M.

Question

Please give Ace some feedback