Lab Electrochemistry

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					                                Lab Electrochemistry

Problem: To determine which metal is more active; how to set-up an electrochemical
cell by labeling the anode and cathode and determining the flow of electrons voltage as
well as determining the voltage when one or more of the concentrations are different
from 1M.

Prelab questions:
   1. Define oxidation and reduction, oxidizing agent and reducing agent.
   2. Using the chart of standard reduction potentials rank the following metals from
       the most active to the least active. Cu, Ag, Na, Mg, Ca, Ni, Pb, Zn
   3. Which of the above metals would be the best reducing agent and why?
   4. Of this group Cu, Cu+2, Na, Na+1 would be the best oxidizing agent? Which
       would be the best reducing agent? Explain your answer.
   5. Rank F, I , Cl, and Br from the most active to the least active nonmetal.
   6. Of this group F, F-1. I, I-1. Which is the best reducing agent? Which is the best
       oxidizing agent? Explain your answer.
   7. On the chart of standard reduction potentials where are the most active metals
       found? The active nonmetals.

Lab Part I :
A Electrochemical Cell using 1M solutions
   1. Set up an electrochemical cell using Cu in 1M Cu(NO3)2 and Al in 1M Al(NO3)3.
   2. Draw the set up labeling the anode, cathode and direction of electron flow.
   3. Write the half-reaction that is occurring at the anode
   4. Write the half-reaction that is occurring at the cathode
   5. Calculate the voltage using the chart of standard reduction potentials
   6. Determine the voltage using a voltage
   7. Calculate the percent error of the cell? What do you think accounts for the
      difference in the numbers?
   A. Electrochemical Cell at varied concentrations
   1. Repeat procedure #1 using 1M Al(NO3)3. and 0.01 M Cu(NO3)2
   2. Calculate the accepted potential using Nernst equation
   3. Determine the voltage of the cell using a volt meter
   4. Calculate the percent error. Give reasons for the difference.

B. Lab Activity series
   1. Place some coiled up copper wire into some silver nitrate and record the results. If
      the reaction is spontaneous, write the half reactions and balance. If it is not
      spontaneous explain why.

   2. Place some coiled up copper wire into some zinc nitrate Place some coiled up
      copper wire into some silver nitrate and record the results. If the reaction is
      spontaneous, write the half reactions and balance. If it is not spontaneous explain
      why.

				
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posted:9/22/2011
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