Complete Lab Report

Inert graphite electrodes were used to create _galvanic cells____ (what were the ions) solutions. A voltage of __9V___ (battery voltage) Volts was applied to _Zinc___ (what electrode?) to create this solution in a previously prepared salt water solution. The salt in the water served as __a device that connects the oxidation and reduction half-cells of a galvanic cell. It maintains the electoral neutrality within the internal circuit___ (why was there salt?) The voltage was applied for __1minute___ (how long or what criteria was used to stop the reaction?)

Galvanic cells of _ iron and aluminum____ (what?) were tested. A reactivity series of these metals was seen to be _____ . This was determined by _____ (explain the criteria used to determine this series’ reactivity)

Concentration cells were tested and a voltage of _____ was found to be between 100% and 10% solutions. The theoretical value of _____ was found by applying the _Nernst____ (what’s the name?) Equation. It was determined that the _____ solution was the oxidation and the _____ solution was the reduction.

Potential errors in the reporting of the voltages could be _____ (explain potential errors. Potential errors are based on the assumptions made. If you say “human error” or “reading the multimeter” then it is -20 for this lab. Think chemically.)

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Record if you altered the procedure in any way.

Insert data tables and pictures here.

· Record visual observations of the anode and solution creation.

· Calculate the expected voltage for each of the combinations

· Insert a picture of all of your prepared solutions and electrodes.

Name this Data Table

Electrolysis was used to create solutions of _____ (name the ions). A voltage of _____ (what did your battery read? Include the unit.) was applied to a metal electrode and _____ (describe the physical observations you witnessed.) To create a copper electrode, a voltage of _____ (battery voltage) was applied for approximately _____ (how long did you wait?). Two _____ (what electrodes did you use to create the copper electrode?) were submerged into a solution of _____ (describe the solution by concentration and species). Table salt was added to all of the solutions _____ (why? This wasn’t explicitly stated. Why would salt need to be a part of each solution?)

Galvanic cells were then tested. _____ (take it from here. Describe the solid / liquid results and propose a reactivity series of these three metals. Look up some sort of theoretical series and discuss if your results match this series. If you believe you have other metals, discuss thoroughly. Explain why the voltmeter was fluctuating. It wasn’t broken and your solutions are fine. Why would the reading vary?)

Three concentration cell scenarios were tested. The original _____ (describe the solution with a concentration) CuSO4 was labeled 100%. A 50/50 dilution with salt water created a solution labeled 50%. A 90/10 dilution (salt water / CuSO4) created a solution labeled 10%. A salt bridge was made by _____ (explain how the salt bridge was formed). _____ electrodes were used to test the voltage between the two solutions. _____ (Take it from here - explain the voltages witnessed.)

Calculations for the theoretical values of the tested concentration cells are provided below.

_____ Insert your theoretical calculations. Include a percent error for your actual results.

Assumptions that were made for this lab include, _____ (insert any assumptions that were made that could have affected the results. Think critically and scientifically. Stating that you assumed “it would work” will be a -10. That is not a scientific assumption.)

The electrochemistry techniques of Electrolysis and Galvanic cells were explored in this lab. _____ Finish the conclusion by stating the broad strokes of the procedure (making anodes and solutions). Including the 100ft view of the results …. What was the reactivity series found? What was the result of the concentration cell part? etc.

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