Define the following terms: electrochemistry, electrochemical cell, salt bridge and redox reactions.

Lab #6 Report Guidelines
Measurement of the Electromotive Force of an Electrochemical Cell

Introduction:
Define the following terms: electrochemistry, electrochemical cell, salt bridge and redox reactions. Explain what an oxidation reaction is and what happens during that type of reaction (do the same for a reduction reaction). Explain what happens with two half-reactions combine. Define/explain Ereduction, Gibbs Energy, EMF, Standard Potential, as well as how one can tell which half-reaction will be reduced/oxidized based off Ereducation. Show (with an equation) how Gibbs Engery and the Standard Potential are related. Explain what a negative/positive means, as well as a large/small . Lastly, explain why it was vital to use solutions with same Molarity in this lab (use an equation to help you with this).

Procedure:
Restate the steps taken to complete this lab in numerical order.

Results:
Include the following:

Also, do a percent error on your calculated value and the measured EMF value for Zinc-Tin.

Discussion/Conclusion:
Restate the purpose of this lab, and state your results. Also, state the percent error for your Zinc-Tin cell. Discuss at least two observations/results from this lab and explain why they occurred. For example, what happened with/without the salt bridge (why was it necessary)? Lastly, be sure to include at least two sources of error.

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