An aluminum half-cell is made with 1.00 x 10-3 M Zn(NO3)3 solution and a zinc electrode. A nickel half cell is made with 1.00 x 10-3 M Ni(C2H2O2)2 solution and a nickel electrode. a. To make a spontaneous voltaic cell, which half-cell needs to undergo oxidation and which half-cell will undergo reduction? Explain why? b. If you were to set up the voltaic cell mentioned in Question 4a, how would you construct your cell. Please indicate which electrode the (+) or the red lead is connected to and what direction are the electrons supposed to flow. c. Describe what is happening at each electrode when the cell is complete. i. anode ii. cathode d. If the the cell bridge is filled a concentrated KNO3 solution, to which half-cell will K+ flow from the salt bridge. Briefly explain. e. Write out the net ionic reaction for the this voltaic cell? f. Predict the voltage generated by this voltaic cell? g. Will you observe the same voltage if the concentration of Ni(NO3) solution is still 1.00 x 10-3 M. Explain why.
An aluminum half-cell is made with 1.00 x 10-3 M Zn(NO3)3 solution and a zinc electrode. A nickel half cell is made with 1.00 x 10-3 M Ni(C2H2O2)2 solution and a nickel electrode.
a. To make a spontaneous voltaic cell, which half-cell needs to undergo oxidation and which half-cell will undergo reduction? Explain why?
b. If you were to set up the voltaic cell mentioned in Question 4a, how would you construct your cell. Please indicate which electrode the (+) or the red lead is connected to and what direction are the electrons supposed to flow.
c. Describe what is happening at each electrode when the cell is complete.
i. anode
ii. cathode
d. If the the cell bridge is filled a concentrated KNO3 solution, to which half-cell will K+ flow from the salt bridge. Briefly explain.
e. Write out the net ionic reaction for the this voltaic cell?
f. Predict the voltage generated by this voltaic cell?
g. Will you observe the same voltage if the concentration of Ni(NO3) solution is still 1.00 x 10-3 M. Explain why.
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