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CHEM 123L – Spring 2018 Sample Final Examination •

YOU DO NOT NEED TO MEMORIZE ANY COMPLEX FORMULAE OR EXTREMELY SPECIFIC FORMULAE: o Below is an example of how the above statement should be interpreted, but is BY NO MEANS a comprehensive list of all the formulae you may need on the final Formulae that you should know: 𝑚 𝑛= 𝑀 𝑞𝑟𝑥𝑛 + 𝑞𝑠𝑜𝑙𝑛 + 𝑞𝑐𝑎𝑙𝑜𝑟𝑖𝑚𝑒𝑡𝑒𝑟 = 0

•

Formulae that you’re not expected to know: 𝑅𝑎𝑡𝑒 = 𝑘[𝐴]𝑚 [𝐵]𝑛 … [𝑍]𝑝

This sample final exam is split into two parts: o Part A is MULTIPLE CHOICE o Part B is SHORT ANSWER

•

THE MULTIPLE CHOICE IN PART A ILLUSTRATES THE TYPES OF QUESTIONS YOU SHOULD EXPECT FROM THE ACTUAL FINAL EXAM o All questions on the actual final will be multiple choice; these questions are meant to teach you how to “test-take” a multiple-choice lab exam!

•

THE SHORT ANSWER IN PART B IS NOT REPRESENTATIVE OF THE ACTUAL FINAL EXAM o There is NO SHORT ANSWER on the actual final; these questions are meant for you to solidify your knowledge of lab skills! If you can answer these questions in your own words, without checking the lab manual, YOU’RE SET!

CHEM 123L Sample Final Exam: Page 2 of 17 Part A – Multiple Choice

General Lab Safety and Knowledge 1. In what section of your lab report does the following paragraph belong? The experimentally-determined value with heat lost to the calorimeter was found to be -43.9 kJ/mol. Compared to the theoretical value of -44.51 kJ/mol, there is a percent error of 1.37%. The relative error can be explained by the assumption that the specific heat of the solution was assumed to be equal to the specific heat of water, which is not true given the concentration of solution used. To improve upon the obtained value, the specific heat of NaOH at a ~1 M concentration should have been used. a) b) c) d) e)

Introduction Materials and Methods Results and Calculations Discussion Conclusion

2. How should the final answer to the following equation be reported? (259 .89 g)(4.184 J g −1 ℃−1)(33.4 − 23.7)℃ ∆𝐻 = 0.247 mol a) b) c) d) e)

4.3 × 104 J/mol 4.27 × 104 J/mol 4.270 × 104 J/mol 4.2703 × 104 J/mol 4.27028 × 104 J/mol

3. Select the one correct OR one incorrect statement concerning proper equipment use: For such questions, either 4 of the options will be correct (true) and 1 of the options will be incorrect (false) OR 4 of the options will be incorrect (false) and 1 of the options will be correct (true). You are expected to pick the ODD ONE OUT. a) Each burette reading should be taken to 2 decimal places and ideally taken with a burette backing card b) The liquid left in the tip of a Mohr pipette is uncalibrated and should not be delivered to your receiving vessel c) When quantitatively transferring a liquid sample to a receiving vessel, you must rinse the dispensing vessel with solvent and transfer the rinsings into the receiving vessel d) To clean the inside of a dirty or wet pipette suction bulb, you must rinse the inside of the bulb with the solution you intend to pipette e) All readings of liquid or solution inside a thin cylindrical vessel (such as a burette or pipette) should be taken with respect to the meniscus

CHEM 123L Sample Final Exam: Page 3 of 17 4. Which of the following is NOT a gross error in laboratory technique? a) Splashing sample solution out of a receiving container by the addition of reagent b) Weighing an object at a different temperature than that of the analytical balance c) Failing to quantitatively transfer all of your sample to the receiving vessel due to improper or not enough rinsing d) Not weighing exactly 25 g of a solid on the top-loading balances when the procedure asks you to weigh 25 grams e) Sucking solution up into the bulb while pipetting, and transferring said solution into the receiving vessel 5. The following methanol molar masses were obtained by three separate trials using the Dumas method: Trial 1 – 45.02 g/mol Trial 2 – 45.06 g/mol Trial 3 – 44.92 g/mol The actual (theoretical) molar mass of methanol is 32.04 g/mol; as such, these results are: a) b) c) d) e)

Neither precise nor accurate Both precise and accurate Accurate but not precise Precise but not accurate There’s a difference between precision and accuracy?

CHEM 123L Sample Final Exam: Page 4 of 17

Experiment 1 – The Dumas Method Useful information: 𝑀𝑚𝑒𝑡ℎ𝑎𝑛𝑜𝑙 = 32.04 g/mol 𝑀𝑖𝑠𝑜𝑝𝑟𝑜𝑝𝑎𝑛𝑜𝑙 = 60.10 g/mol

𝑀𝑒𝑡ℎ𝑎𝑛𝑜𝑙 = 46.07 g/mol 𝑀ℎ𝑒𝑥𝑎𝑛𝑒 = 86 .18 g/mol

6. Select the one correct OR one incorrect statement related to the Dumas Method: a) One of the main assumptions of the Dumas method is that all of the liquids behave ideally when in the vapour form b) During the experiment, needles were used as a channel that would equalize the internal vessel pressure to the external vessel pressure c) The mass of the volatile vapour remaining in the vessel was used to determine the molar mass of the liquid being analyzed, in that the vessel was weighed right after removal from the hot water bath d) Ignoring any excess condensed liquid left in the vessel between trials does NOT introduce any error with respect to the experimentally-determined results e) By using the results obtained in the Dumas Method, you could theoretically confirm the identity of an unknown volatile liquid based on its molar mass Use the following information to answer question 7: The Dumas Method was employed to determine the experimental molar masses of four volatile liquids; the results of the experiment can be seen below: Volatile Liquid Methanol Ethanol Isopropanol Hexane

Experimental Molar Mass (g/mol) 29.38 52.81 82.06 107.85

7. What conclusions can be drawn from the obtained data? a) The Dumas method seems to be significantly less accurate when determining the molar masses of larger compounds b) The experimental molar mass of methanol being lower than theoretical could be explained by the fact that not all of the vapour trapped in the vessel condensed back into liquid to be massed c) The experimental molar masses of ethanol, isopropanol, and hexane being much higher than theoretical can be explained by the fact that the temperature recorded was higher than the actual temperature by a couple of degrees d) a and b e) a, b, and c

CHEM 123L Sample Final Exam: Page 5 of 17 8. A student running a methanol trial for the Dumas Method has pulled their vessel out from the hot water bath and has submerged it within the ice bath; the vessel has been in the ice bath for 2 minutes. Which of the following are present in the vessel at this time? i. Methanol (l) ii. Methanol (g) iii. Methanol (aq) iv. Air (g) v. 𝐻2 𝑂(l) a) i. b) i. and ii. c) i. ii. and iii. d) i. ii. and iv. e) i. iv. and v. 9. Below is a list of substances and their normal melting and boiling points: Substance T W X Y Z

Melting Point (℃) -5.6 48.2 16.4 -58.4 0.0

Boiling Point (℃) 35.8 87.9 112.6 65.4 100.0

For which of the listed substances could you easily determine a molar mass using the Dumas method? a) T, W, and Y b) X and Y c) T and Y d) W and Z e) T, Y, and Z

CHEM 123L Sample Final Exam: Page 6 of 17 10. Using the data set below, calculate the average molar mass of ethanol across all trials. The ideal gas constant is 8.3145 kPa ∙ L ∙ mol−1 ∙ K −1 Trial No. 1

2

3

Vessel

Volume of Vessel (L)

Flask

Mass of Condensed Liquid (g) 0.2743

Test Tube

0.06350

0.03512

100.7

103.0

Flask

0.2745

0.15056

100.7

103.0

Test Tube

0.06350

0.03512

100.7

103.0

Flask

0.2663

0.15056

100.7

103.0

Test Tube

0.06360

0.03512

100.7

103.0

The average molar mass is: a) b) c) d) e)

54.46 g/mol 53.8 g/mol 54.49 g/mol 54.60 g/mol 54.53 g/mol

0.15056

Temperature Barometric (℃) Pressure (kPa) 100.7 103.0

Experimental Molar Mass (g/mol)

CHEM 123L Sample Final Exam: Page 7 of 17

Experiment 2 – Introduction to Calorimetry 11. The following units: 𝑘𝐽 𝑚𝑜𝑙 correspond to which variables respectively? a) 𝑞𝑟𝑥𝑛 , ∆𝐻𝑛𝑒𝑢𝑡 , ∆𝑇, 𝐶𝑐𝑎𝑙 , 𝑠𝑠𝑜𝑙𝑛 b) ∆𝑇, 𝐶𝑐𝑎𝑙 , 𝑠𝑠𝑜𝑙𝑛 , ∆𝐻𝑠𝑜𝑙𝑛 , 𝑞𝑟𝑥𝑛 c) ∆𝑇, 𝐶𝑐𝑎𝑙 , 𝑞𝑐𝑎𝑙 , ∆𝐻𝑠𝑜𝑙𝑛 , 𝑠𝑤𝑎𝑡𝑒𝑟 d) ∆𝑇, 𝑞𝑠𝑜𝑙𝑛 , 𝐶𝑐𝑎𝑙 , 𝑠𝑤𝑎𝑡𝑒𝑟 , ∆𝐻𝑟𝑥𝑛 e) ∆𝑇, ∆𝐻𝑛𝑒𝑢𝑡 , 𝑠𝑠𝑜𝑙𝑛 , 𝐶𝑐𝑎𝑙 , 𝑞𝑐𝑎𝑙 𝐾

𝐽 𝑔℃

𝐽 ℃

𝐽

12. Below is a plot made for the determination of the calorimeter’s heat capacity. Using only the information found on the plot, determine 𝐶𝑐𝑎𝑙 , the calorimeter constant (assume that the hot water was found in the calorimeter before the cool water was added). Temperature Readings for the Mixing of Hot and Cool Water for the Determination of the Calorimeter Constant, Ccal

Plot 1.

60.0

51.0 oC 49.5 oC 50.0

Temperature (℃)

40.0

34.1 oC

30.0

33.1 oC 21.0 oC

20.0

𝑚ℎ𝑒𝑎𝑡𝑒𝑑 𝑤𝑎𝑡𝑒𝑟 = 113.76 g 𝑚𝑐𝑜𝑜𝑙 𝑤𝑎𝑡𝑒𝑟 = 176.56 g 𝑠𝑤𝑎𝑡𝑒𝑟 = 4.184 J g

−1

10.0

Reaction's Temperature Curve

−1

℃

Initial Temperature of Cool Water 0.0

-8

-6

-4

-2

0

2

Time (minutes)

a. b. c. d. e.

69.1 J/oC 96.7 J/oC 23.4 J/oC 152 J/oC 111 J/oC

4

6

8

10

12

CHEM 123L Sample Final Exam: Page 8 of 17

13. Given the following reaction: 𝐾𝐶𝑙𝑂3 (s) → 𝐾 + (aq) + 𝐶𝑙𝑂3− (aq) Calculate the enthalpy of solution per mole of reaction if 4.98 grams of solid KClO3 (molar mass of 122.55 g/mol) is dissolved in 260.00 mL of water at 22.3 oC. The final temperature of the reaction is 294.0 K. Assume that the specific heat of the solution is equal to that of water, the density of water is 1 g/mL, and include a correction for the heat lost to the calorimeter, assuming that Ccal = 73.2 J/oC. a. b. c. d. e.

42.2 kJ/mol 39.6 kJ/mol 1.71 kJ/mol -42.2 kJ/mol -1.71 kJ/mol

14. For the following neutralization reaction (same as the one you performed in the Lab): 𝑁𝑎𝑂𝐻(aq) + 𝐻𝐶𝑙(aq) → 𝑁𝑎𝐶𝑙(aq) + 𝐻2 𝑂(l)

∆𝐻𝑛𝑒𝑢𝑡 = −55.90 kJ/mol of H2 O(l)

When 100 mL of ~1 M NaOH was reacted with 150 mL of 1.036 M HCl, you calculated an enthalpy of neutralization, ∆𝐻𝑐𝑎𝑙𝑐𝑢𝑙𝑎𝑡𝑒𝑑 . Which of the following assumptions does not allow you to successfully calculate [NaOH]? a.

∆𝐻𝑐𝑎𝑙𝑐𝑢𝑙𝑎𝑡𝑒𝑑 𝑥 mol H2 O

b. c. d. e.

𝑛𝑁𝑎𝑂𝐻 = 𝑛𝐻2 𝑂 𝑛𝐻𝐶𝑙 = 𝑛𝐻2 𝑂 The heat lost to the calorimeter is negligible The reaction goes to completion

= ∆𝐻𝑛𝑒𝑢𝑡

15. Select the one correct OR one incorrect statement regarding calorimetry a. In performing the calorimetry calculations, there is no heat lost to, or gained from the environment b. It is impossible to determine the specific heat of a substance using calorimetric methods c. Calorimetry relies on using a calorimeter to measure the heat stored by substances and any changes in temperature in a chemical or physical process d. The change in temperature of the calorimeter is also the change in temperature of the substance added to the calorimeter e. It is impossible to determine the specific heat of a multicomponent object such as a calorimeter because it is impossible to account for all the components

CHEM 123L Sample Final Exam: Page 9 of 17

Experiment 3 – The Iodide-Persulfate Reaction Useful information and chemical equations: 𝑆2 𝑂8 2− + 2𝐼− → 𝐼2 + 2𝑆𝑂4 2− 𝐼2 + 2𝑆2 𝑂3 2− → 2𝐼− + 𝑆4 𝑂6 2− −∆[𝑆2 𝑂8 2− ] = 𝑘[𝑆2 𝑂8 2− ][𝐼 − ] Rate law for Equation 1: 𝑅𝑎𝑡𝑒 = ∆𝑡 𝐸𝑞𝑢𝑎𝑡𝑖𝑜𝑛 1: 𝐸𝑞𝑢𝑎𝑡𝑖𝑜𝑛 2:

16. For a given chemical reaction, the rate law using arbitrary solutions, A(aq) and B(aq), is: 𝑅𝑎𝑡𝑒 = 𝑘[𝐴][𝐵]2 What are the units of the rate constant, k, assuming the concentrations of the solutions are given in mol/L? a. L ∙ mol−1 ∙ s −1 b. mol ∙ L−1 ∙ s −1 c. L2 ∙ mol−2 ∙ s −1 d. L2 ∙ mol−2 e. s ∙ mol−1 ∙ L−1 17. A student has forgotten to add one of the components to the Iodide-Persulfate mixture (oh no!). After 3 minutes, the mixture was observed to be yellow in colour; after 5 minutes, the mixture was observed to be a deep wine colour. Using your knowledge of the experiment, what component did the student forget to add? a) Potassium iodide b) Starch c) Sodium thiosulfate d) a and b e) a, b, and c 18. In which of the following scenarios would you expect the rate of the Iodide-Persulfate reaction to INCREASE, assuming nothing else about the reaction is changed in the given scenario? i. An increase in temperature ii. A decrease in ionic strength iii. Increasing the concentration of persulfate in the reaction mixture iv. Decreasing the concentration of iodide in the reaction mixture a) i. only b) ii. only c) iv. only d) i. and iii. e) i. iii. and iv.

CHEM 123L Sample Final Exam: Page 10 of 17 19. Given below is data from a trial of the Iodide-Persulfate reaction conducted by a CHEM 123L student last term; the substances added to a reaction vessel in their respective concentrations and volumes are seen: Substance: (aq) Concentration: (M) Volume Added: (mL)

(𝑁𝐻4 )2 𝑆2 𝑂8 (𝑁𝐻4 )2 𝑆𝑂4

𝐾𝐼

𝐾𝑁𝑂3

𝑁𝑎2 𝑆2 𝑂3

𝑆𝑡𝑎𝑟𝑐ℎ

0.100

0.100

0.200

0.200

0.0100

N/A

20.0

0

10.0

10.0

10.0

5.0

This student recorded the time taken to see a colour change as 210.55 seconds. What is the reaction rate for this trial? a. b. c. d. e.

2.37 × 10−4 mol ∙ L−1 ∙ s −1 4.32 × 10−6 mol ∙ L−1 ∙ s −1 4.75 × 10−4 mol ∙ L−1 ∙ s −1 4.75 × 10−5 mol ∙ L−1 ∙ s −1 8.64 × 10−5 mol ∙ L−1 ∙ s −1

20. Select the one correct OR one incorrect statement about the Iodide-Persulfate Reaction experiment: a) Changing the ionic strength of the reaction mixture will change the rate of the reaction and the rate constant b) It is only when all of the thiosulfate added to the reaction mixture is used up in the chemical reaction that the colour of the solution changes from clear to coloured c) The rate law for the iodide-persulfate reaction is first order with respect to the persulfate and first order with respect to the iodide d) Starch is being added as an indicator to the reaction mixture so that the solution turns a yellow colour when starch is present rather than blue when starch is absent e) A reason the reaction might never change colour is forgetting to add potassium iodide to the reaction mixture

CHEM 123L Sample Final Exam: Page 11 of 17

Experiment 4 – pH Chemistry Useful Equations: Henderson − Hasselbalch Equation: 𝐾𝑎 =

[𝐻+ ][𝐴− ] [𝐻𝐴]

𝐾𝑏 =

𝑝𝐻 = 𝑝𝐾𝑎 + log

[𝐴− ] [𝐻𝐴]

[𝑂𝐻− ][𝐻𝐵] [𝐵− ]

21. Select the one correct OR one incorrect statement based on pH chemistry: a. The Bronsted-Lowry definition of an acid is a substance that relinquishes (donates) protons b. The pH meters used in the lab indicate the pH by measuring the electromotive force generated through using the solution as an electrolyte c. In this reaction: 𝐶𝐻3 𝑁𝐻3+ (𝑎𝑞) + 𝐻2 𝑂(𝑙) ⇄ 𝐶𝐻3 𝑁𝐻2 (𝑎𝑞) + 𝐻3 𝑂+ (𝑎𝑞 ), the methylammonium ion 𝐶𝐻3 𝑁𝐻3+ , is the acid and the methylamine, 𝐶𝐻3 𝑁𝐻2 , is its conjugate base d. Buffers with a higher concentration have the tendency to resist more changes in pH as they can neutralize more of the acid/base added to it before depletion e. The concentration ratio

[𝐻𝐴] [𝐴−]

is called the buffer ratio

Use the following information to answer questions 22 and 23: When performing a weak acid-strong base titration, 50.00 mL of 0.1320 M acetic acid, CH3COOH, is titrated with 0.1650 M potassium hydroxide, KOH. The pKa of acetic acid is 4.76 22. What is the pH of the acetic acid solution after the addition of 7.00 mL of KOH? a. 3.86 b. 4.09 c. 4.84 d. 5.43 e. 5.66 23. What is the pH of the acetic acid solution after the addition of 20.00 mL of KOH? a. 3.95 b. 4.43 c. 4.76 d. 4.84 e. 5.09

CHEM 123L Sample Final Exam: Page 12 of 17 24. You have made a 50.0 mL buffer composed of 25.0 mL of 1.002 M ammonia (NH3) and 25.0 mL of 1.038 M ammonium nitrate (NH4NO3). What is the pH of the buffer BEFORE the addition of 5.0 mL of 2.0 M HCl, and AFTER the addition? The pKb for NH3 is 4.75 a. 𝑝𝐻𝑏𝑒𝑓𝑜𝑟𝑒 = 4.73 𝑝𝐻𝑎𝑓𝑡𝑒𝑟 = 4.37 b. 𝑝𝐻𝑏𝑒𝑓𝑜𝑟𝑒 = 4.77 𝑝𝐻𝑎𝑓𝑡𝑒𝑟 = 5.13 c. 𝑝𝐻𝑏𝑒𝑓𝑜𝑟𝑒 = 7.02 𝑝𝐻𝑎𝑓𝑡𝑒𝑟 = 6.91 d. 𝑝𝐻𝑏𝑒𝑓𝑜𝑟𝑒 = 9.23 e. 𝑝𝐻𝑏𝑒𝑓𝑜𝑟𝑒 = 9.27

𝑝𝐻𝑎𝑓𝑡𝑒𝑟 = 8.87 𝑝𝐻𝑎𝑓𝑡𝑒𝑟 = 9.63

25. Select the one correct OR incorrect statement based on the titration curve seen below:

Plot 2:

Effects on pH during a Titration with Methyl Red as the Indicator

12.00

Titration Curve Half-Neutralization Point 10.00

Point C

Indicator Colour Change

8.00

pH of Solution

Region X 6.00 5.50

Indicator Transition Range: pH = 4.8 to 6.0

Point A: 𝑛𝑎𝑐𝑖𝑑 = 𝑛𝑏𝑎𝑠𝑒

4.00

Point B 2.00

0.00 0

5

10

15

20

24.1025

30

35

40

45

Volume of Titrant Added (mL)

a. “Region X” denotes the buffer region (area where buffering is occurring) b. The half-neutralization point (Point C) is a special point where the pKa of the titrant is equal to the pH of the solution to which it is being added c. In this titration, a weak acid was titrated with a strong base d. The point at which indicator colour change was observed (Point B) is also called the “equivalence point” e. Methyl red is NOT a suitable indicator for this titration because Point A and Point B both lie within the indicator’s transition range

CHEM 123L Sample Final Exam: Page 13 of 17

Experiment 5 – Electrochemistry Useful Information and Equations: Nernst Equation:

𝑜 − 𝐸𝑐𝑒𝑙𝑙 = 𝐸𝑐𝑒𝑙𝑙

0.0592 log10 𝑄 𝑛

Table 1: Some Standard Reduction Potentials Reaction Number 1 2 3 4 5 6 7 8 9

Half-Reaction Ag + 1e− → Ag(s) Fe3+ (aq) + 1e− → Fe2+ (aq) Cu2+ (aq) + 2e− → Cu(s) 2H+ (aq) + 2e− → H2 (g) Pb2+ (aq) + 2e− → Pb (s) Ni2+ (aq) + 2e− → Ni (s) Cd2+ (aq) + 2e− → Cd (s) Fe2+ (aq) + 2e− → Fe (s) Zn2+ (aq) + 2e− → Zn (s) + (aq)

Eo (V) 0.80 0.77 0.34 0.00 -0.13 -0.25 -0.40 -0.44 -0.76

26. Select the one correct OR one incorrect statement using only the information in Table 1: a) The strongest reducing agent is Ag+ (aq) b) Fe (s) would be spontaneously oxidized to Fe2+ (aq) by Ni2+ (aq) c) Assuming only standard conditions, the smallest standard cell potential that can be produced in a working spontaneous cell is obtained by combining half-reactions 4 and 5 d) Pb2+ (aq) would be spontaneously reduced to Pb (s) by Cu (s) e) Cd2+ (aq) would be spontaneously oxidized to Cd (s) by Fe3+ (aq) 27. For the following electrochemical cell, which is the correctly-balanced chemical reaction and correct cell potential? 𝑃𝑏(s) ǀ 𝑃𝑏(𝑁𝑂3 )2 (0.18 M, aq) ǁ 𝐹𝑒 3+ (1.5 M, aq), 𝐹𝑒 2+ (0.23 M, aq) ǀ 𝑔𝑟𝑎𝑝ℎ𝑖𝑡𝑒(s) a) b) c) d) e)

𝑃𝑏(𝑠) + 𝐹𝑒 3+ (𝑎𝑞) → 𝐹𝑒 2+ + 𝑃𝑏(𝑁𝑂3 )2 (𝑎𝑞 ); 𝐸𝑐𝑒𝑙𝑙 = 0.90 V 3+ (𝑎𝑞) 2+ 𝑃𝑏(𝑠) + 𝐹𝑒 → 𝐹𝑒 + 𝑃𝑏(𝑁𝑂3 )2 (𝑎𝑞); 𝐸𝑐𝑒𝑙𝑙 = 0.99 V 3+ (𝑎𝑞) 2+ ( 𝑃𝑏(𝑠) + 2𝐹𝑒 → 2𝐹𝑒 𝑎𝑞) + 𝑃𝑏(𝑁𝑂3 )2 (𝑎𝑞); 𝐸𝑐𝑒𝑙𝑙 = 0.90 V 2+ 3+ ( ) (𝑎𝑞) (𝑎𝑞) (𝑎𝑞) ) 𝑃𝑏 𝑁𝑂3 2 + 𝐹𝑒 → 𝐹𝑒 + 𝑃𝑏(𝑠 ; 𝐸𝑐𝑒𝑙𝑙 = 0.81 V 𝑃𝑏(𝑠) + 2𝐹𝑒 3+ (𝑎𝑞) → 2𝐹𝑒 2+ (𝑎𝑞) + 𝑃𝑏(𝑁𝑂3 )2 (𝑎𝑞); 𝐸𝑐𝑒𝑙𝑙 = 0.97 V

CHEM 123L Sample Final Exam: Page 14 of 17 28. A reagent, Compound X, is added to the anode’s electrolyte solution of the cell (seen below) so that it reacts with the Fe2+...