A student made measurements on some electrochemical cells and calculated three quantities:. The standard reaction free energy AGO.• The equilibrium constant K at 25.0 °C.• The cell potential under standard conditions EºHis results are listed below.olo10ArUnfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any.Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity iscorrect.Also note: for each cell, the number n of electrons transferred per redox reaction is 1.calculated quantities(Check the box next to any that are wrong.)cell00AG18A108. kJ/mol8.33 x 10-130. kJ/mol5.96 x 10B1Ho-1.12 V-1.35 VOO4D Also note: for each cell, the number n of electrons transferred per redox reaction is 1.calculated quantities(Check the box next to any that are wrong.)cell n00AGK18A1108. kJ/mol O8.33 x 10B- 130. kJ/mol5.96 × 10C-116. kJ/mol O4.76 × 101122-21OOXE-1.12 V-1.35 V1.20 VS?OOO

Answered: Image /qna-images/answer/66ebab25-3c42-4055-82bb-2903ca87002e.jpg

Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell 12. AG K R 1 A 18 8.33 x 10 O 108. kJ/mol O -1.12 V 22 B -130. kJ/mol O 5.96 x 10 O -1.35 V -116 kJ/mol O 4.76 10 1.20 V C 1 1 -21 O X S ? O O O

Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell 12. AG K R 1 A 18 8.33 x 10 O 108. kJ/mol O -1.12 V 22 B -130. kJ/mol O 5.96 x 10 O -1.35 V -116 kJ/mol O 4.76 10 1.20 V C 1 1 -21 O X S ? O O O

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Answer the following questions using the data in Appendix L of the textbook. a. Calculate the standard cell potential for a galvanic cell made with Ni and Ag. b. Calculate the standard cell potential for a galvanic cell made with Ni and Zn.
How is the amount of current flowing through an electrolytic cell related to the amount of product produced in the redox reaction? Match the items in the left column to the appropriate blanks in the sentences on the right. multiplied coulombs Avogadro's 1 mol Faraday's 1g ampers 6.022 x 10¹ mol volts divided The number of moles of electrons that have flowed in a given electrolysis cell can be determined by measuring the total charge that has flowed through the cell. If the amount of current flowing through the cell is by the time that the current flowed, the total charge that passed through the cell in that time can be found. The relationship between charge and the number of moles of electrons constant, which corresponds to the charge in is given by of of electrons. These relationships are used to solve problems involving the stoichiometry of electrolytic cells. Reset Help
1. Use the standard reduction potentials in the table to create a galvanic cell with the highest possible standard cell voltage. a. Write the oxidation half-reaction. b. Write the reduction half-reaction. c. Calculate the standard cell voltage. d. Write the overall cell reaction (redox reaction)
A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H (aq) +Se Fe³+ (aq) +e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. half-reaction Write a balanced. equation for the Answer the following questions about this cell. 0 - Mn² (aq) + 4H₂O(1) Fe (aq) standard reduction potential +1.51 V Ered=+0.771 V 20 "red =
A layer of chromium is electroplated on an automobile bumper by passing a constant current of 40.0 A through a cell that contains Cr3+(aq). How many hours are required to deposit 151 g of chromium? Note: Electroplating is the formation of a metal by the reduction of a metal cation. Select one: a. 32.7 h b. 58.4 h c. 5.84 h d. 3.27 h e. 19.5 h f. 1.95 h
Calculate the concentration of an unknown solution in a concentration cell. A concentration cell consisting of two hydrogen electrodes (P H2- latm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.193 V. What is the pH in the unknown solution? Assume the temperature of the solutions is 298 K. !! pH =
78. A voltaic cell consists of a Pb/Pb2 half-cell and a Cu/Cu2" half- cell at 25 C. The initial concentrations of Pb and Cu are 0.0500 M and 1.50 M, respectively. a. What is the initial cell potential? b. What is the cell potential when the concentration of Cu2" has fallen to 0.200 M? c. What are the concentrations of Pb- and Cu" when the cell potential falls to 0.35 V?
Which of the following statements is(are) true for all galvanic cells? 1. Reduction occurs at the cathode. II. The anode gains mass during discharge (note: this means operation of the cell.) III. The voltage is less than or equal to zero. O only I O only III O only II O L I, and II O Il and II
1) Construct a zinc-copper electrochemical cell using 1.0 M Zn2+ and 1.0 M Ni2+ solutions. a. Provide the shorthand notation. b. What is the EMF of this cell (include units)? c. For the voltage that you are measuring, is this E°cell or Ecell? Explain.
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl solution - a Ni electrode in 1.0 M Ni(NO) solution When the cell is running spontaneously, which of the choices are true? a.) The nickel electrode gains mass and the nickel electrode is the cathode. b.) The nickel electrode loses mass and the nickel electrode is the cathode. c.) The iron electrode gains mass and the iron electrode is the anode. d.)The iron electrode loses mass and the iron electrode is the cathode.
Balance each redox reaction occurring in acidic aqueous solution.a. I-(aq) + NO2-(aq)---->I2(s) + NO( g)b. ClO4-(aq) + Cl-(aq)----->ClO3-(aq) + Cl2( g)c. NO3-(aq) + Sn2+(aq)------>Sn4+(aq) + NO( g)
3. The Eel fora galvanic cell composed of a Li electrode and an unknown electrode was found to be 2.91 volts. Use the Standard Reduction Potential table to determine the identity of the unknown electrode. Show work. Ered (Volts) -0.80 -0.34 -0.04 -0.76 -0.14 -0.40 -2.37 Half-Reaction Ag (aq) + 1e → Ag(s) Cu²+ (aq) + 2e > Cu(s) Fe (aq) + 3e > Fe(s) Zn²+ (aq) Sn²+ (aq) + 2e +2e → Zn(s) Sn(s) Cd²+ (aq) + 2e* Cd(s) Mg²+ (aq) + 2e Mg(s)