Electrochemistry Simulations Experiment 9 Paper

Question Description

write down observations first, and answer all the questions.

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Experiment 9: Electrochemistry Simulations In this experiment you will be working with a computer simulation that covers electrochemistry, please consider each experiment carefully, write down your observations, and answer the questions to the best of your ability. Part 1. Activity Series When metals lose electrons they form metal cations, which go into solution. This process is called oxidation. Thus we might say that Na oxidizes to Na+ when we put it in water. When a metal oxidizes it gradually dissolves (the cation is soluble in water). When a metal cation gains electrons (a reduction process) then the metal plates out on the surface of the reduction site. When a metal is placed in contact with a solution of a different metal cation, the more active metal (more easily oxidized) goes into solution. If the more active metal is already in solution as the cation there is no observable reaction. You will look at a series of metals in contact with solutions of other metal ions to establish an activity series, that is, a determination of which metal is most active, next most active, etc. To access the simulation go to the web site below. redox simulation To start the simulation click on the start button and then select Activity 1. You will see four ionic solutions. Select magnesium metal and follow the instructions on the screen. Write down your observations (e.g. what reaction occurred) for magnesium in each of the solutions. Repeat the procedure for copper, zinc, and silver, recording your observations each time. Use the observations from your experiments to answer the following questions: 1. Which of the four metals you tested is the most reactive. Explain why. 2. Which of the four metals you tested is the least reactive. Explain why. 3. Arrange the metals in order of increasing reactivity (from the least reactive to the most reactive). Part 2. Electrochemical Cells In this part of the experiment you are going to construct a zinc-copper electrochemical cell. Use the link below to access the web site and begin by assembling a zinc-copper cell. Each half-cell should consist of a metal electrode in contact with a solution of its ions. Check from Part 1 to select a reaction that will give a positive cell potential, that is, a spontaneous electrochemical reaction. The anode is the electrode at which oxidation occurs and will be negative (black wire). The cathode is the electrode at which reduction occurs and will be positive (red wire). If you get a negative potential when you operate your battery you have connected your electrodes up in the wrong order. Please be sure to follow the instructions on the screen. electrochemical cell simulation As you are running the simulation you might want to answer the following questions: 1. Is there an electron transfer between species? 2. Which species is losing electrons? 3. Write down the half reaction for the species that is undergoing oxidation (losing electrons). 4. Which species is gaining electrons? 5. Write down the half reaction for the species that is undergoing reduction (gaining electrons). 6. Which metal is the anode? 7. Which metal is the cathode? 8. Is this a spontaneous process? Explain your reasoning. 9. Write the complete balanced equation for the reaction, that is, the sum of the two half-reactions. After you have answered all the questions be sure to go to the Quizzes page to report your experiment results to your instructor. ...
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Final Answer

Hello there!Here is the solution 😇

Part 1:
Mg(NO3 )2

Zn(NO3 )2

𝐶𝑢 (NO3 )2


Oxidation reaction
occurred to Mg
and Zn
precipitated on the
bar of Mg (Zn is
No reaction

Oxidation reaction
occurred to Mg and
Cu precipitated on
the bar of Mg (Cu is

Oxidation reaction

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