Lab #6 Report Guidelines
Measurement of the Electromotive Force of an Electrochemical Cell
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).
Restate the steps taken to complete this lab in numerical order.
Include the following:
Also, do a percent error on your calculated value and the measured EMF value for Zinc-Tin.
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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