The ChemCollective   NSDL and CMU

Electrochemistry

-Introduction

Step 1:

-Investigating redox reactions

-Practice with redox reactions

-Reduction tendencies of metal ions

Step 2:

-Electron transfer

-Electrochemical cell

-Practice with cells

-Powering a stopwatch

Step 3:

-Measuring potentials

-Calculating potentials

-Practice with potentials

-Applying potentials

Step 4:

-Non-standard conditions

-Practice with non-standard cells

Feedback Form:

-Download Activity Form



Electrochemistry Tutorial: Galvanic Cells and the Nernst Equation >> Step 4: Practice with cells in non-standard conditions

  < Previous

Electrochemistry: Galvanic Cells and the Nernst Equation

Step 4: Practice with cells in non-standard conditions

Please use the feedback form to answer the following questions which will be turned in to your TA.

Activity: Determine the effects of changing half-cell concentration on cell potential.
Use the simulation below to explore the effects of changing half-cell concentrations and to answer the following questions.

  1. Dilute the Sn2+ solution in the following two galvanic cells. What happens to the voltage in each? Explain your results.
    1. Reaction 1:       Sn(s) + Cu2+(aq) --> Sn2+(aq) + Cu(s)
    2. Reaction 2:       Zn(s) + Sn2+(aq) --> Zn2+(aq) + Sn(s)

  2. Consider a cell: Zn(s) + Cu2+(aq) --> Zn2+(aq) + Cu(s) in which the concentration of [Cu2+] and [Zn2+] are both 2M. [Note that the simulation does not provide solutions above 1M. Please make predictions about cells with 2M concentrations based upon experiments you perform with the concentrations provided.]
    1. Will the cell potential be greater than, equal to or less than the standard cell potential?
    2. Will the cell be able to run the stopwatch for a longer time, equal time, or shorter time than the standard cell?


Get Adobe Flash player

This concludes the electrochemistry activity, please be sure to complete the activity form.

  < Previous

   Page Last Updated: 11.07.2016