Use Table 1 as a source of half-equations and reduction potentials for this assignment. 1. Rank the following metals by ease of oxidation, from hardest to easiest: Cu; aluminum, Al; Fe; and chromium, Cr. 2. An Al strip is placed in CuSO4 solution. a. Would you expect a spontaneous reaction to occur, based on the net potential? b. If your answer to (1) is "yes," what would you observe? c. Write a chemical equation that describes your predicted observations. Table 1 Selected standard reduction potentials for half-reactions red measured in Reduction Half-Equation E° red, V Mg2+(aq) + 2e→ Mg(s) -2.37 Al3+(aq) + 3 e → Al(s) -1.66 Cr²+(aq) + 2e → Cr(s) -0.91 Zn2+(aq) + 2e → Zn(s) -0.76 Fe2+(aq) + 2e → Fe(s) -0.44 Ni²+(aq) + 2e → Ni(s) -0.26 Sn2+(aq) + 2e → Sn(s) -0.14 Pb2+(aq) + 2 e → Pb(s) -0.13 2 H+(aq) + 2e → H2(g) 0.00 Cu2+(aq) + 2e→ Cu(s) +0.34 Ag+(aq) + e Ag(s) +0.80

Use Table 1 as a source of half-equations and reduction potentials for this assignment. 1. Rank the following metals by ease of oxidation, from hardest to easiest: Cu; aluminum, Al; Fe; and chromium, Cr. 2. An Al strip is placed in CuSO4 solution. a. Would you expect a spontaneous reaction to occur, based on the net potential? b. If your answer to (1) is "yes," what would you observe? c. Write a chemical equation that describes your predicted observations. Table 1 Selected standard reduction potentials for half-reactions red measured in Reduction Half-Equation E° red, V Mg2+(aq) + 2e→ Mg(s) -2.37 Al3+(aq) + 3 e → Al(s) -1.66 Cr²+(aq) + 2e → Cr(s) -0.91 Zn2+(aq) + 2e → Zn(s) -0.76 Fe2+(aq) + 2e → Fe(s) -0.44 Ni²+(aq) + 2e → Ni(s) -0.26 Sn2+(aq) + 2e → Sn(s) -0.14 Pb2+(aq) + 2 e → Pb(s) -0.13 2 H+(aq) + 2e → H2(g) 0.00 Cu2+(aq) + 2e→ Cu(s) +0.34 Ag+(aq) + e Ag(s) +0.80

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

An electrochemical cell uses Ag and Zn as electrodes. Based on the reduction potentials, the (blank) electrode is where the reduction will occur and it is called the (blank) a.Ag, cathode b.Zn, anode c.Ag, anode Based on the reactions below, which is the stongest reducing agent? +1.22 V MnO2(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H2O(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2- (aq) -0.95 V SnO2(s) + 2H2O() + 4e-→ Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- → Cr(s) + 3OH-(aq) a.Hg2SO4 b.Mn02 c.Cr d.Sn e.Hg Identify the strongest oxidizing agent from the following half-reactions. The standard reduction potentials are listed. +1.22 V Mn02(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H20(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2-(aq) -0.95 V SnO2 (s) + 2H2O() + 4e- Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- Cr(s) + 3OH- (aq) a. MnO2 b.Hg2SO4 c.Sn d.Hg e.Cr
PART II) -Q1 for the following Redox reaction: Co, + 2H > Co* + Haa) (aq) 1) Draw a detailed diagram of the cell: anode, cathode, salt bridge and the direction flow of the electrons.{Remember Co is one of the two electrodes & S.H.E. is the other electrode}
62
2. Using the available materials, design a spontaneous electrochemical cell at standard conditions with initial E° of +0.90V. a. Label the anode and cathode metals b. Label the anode and cathode solutions c. Draw arrows through the wire to indicate the direction of electron flow d. Indicate which ion from the salt bridge will migrate into each chamber e. Write the balanced half-reactions for each electrode and the overall balanced equation f. Circle whether each electrode will increase or decrease in mass g. Indicate the value of n, the number of electrons/mole rxn, in the balanced equation h. Calculate AG° electron flow KNO anode metal cathode metal anode solution _cathode solution ion migration anode half reaction cathode half reaction electrode mass: increases or decreases electrode mass increases or decreases overall balanced equation: n=
QUESTION 1 Match the following terms to the correct definition. standard reduction potential (E°) Anode Cathode oxidation half-reaction Galvanic cell Cell potential reduction half-reaction electrical potential - A. difference in electrical potential that arises when dissimilar metals are connected; the driving force for the flow of charge (current) in oxidation-reduction reactions B. "the half of an oxidation-reduction reaction involving oxidation; the half-reaction in which electrons appear as products; balanced when each atom type, as well as the charge, is balanced" C. electrode in an electrochemical cell at which oxidation occurs; information about the anode is recorded on the left side of the salt bridge in cell notation D. electrochemical cell that involves a spontaneous oxidation-reduction reaction; electrochemical cells with positive cell potentials; also called à voltaic cell E. "energy per charge; in electrochemical systems, it depends on the way the charges are distributed…
1. a. In one half-cell of a galvanic cell, a piece of platinum metal, Pt, dips into a solution containing 0.850 M Fe * and 0.010M Fe 2*. In the other half-cell a piece of cadmium metal, Cd, dips into a 0.500 M solution of Cd 2*. €° = +0.771 V for Fe * + e 2 Fe * e° = -0.403 V for Cd 2* + 2 e 2 cd i. Write the shorthand notation for the cell. ii. Calculate the standard cell potential, ɛ°. ii. Calculate the equilibrium constant for the cell reaction. iv. Calculate the cell potential, ɛ. b. The oxidation of ethanol by the permanganate ion, MnO, in aqueous acidic solution produces ethanoic acid and Mn²*. Use the half reaction method and write the balanced equation for this reaction.
1. Balance the following redox reactions using the half-cell method, assume acidic solution. a. Fe3+ + H2S Fe2+ + H+ + S b. Pb(OH)4² + BrO PbO2 + Br C. MnO4 + H2O2 Mn2+ + O2
For a Magnesium-Aluminum cell [Mn2+ + 2e- --> Mn (-1.18V)] [Al3+ + 3e- --> Al (-1.66)]: 1. label anode, cathode2. write half reactions3. Write overall reaction4. Write cell notation5. Calculate E6. Calculate G = -nFe7. Show and give example of how G is related to K8. Calculate Nernst for various Molarity changes (show how E changes)9. Calculate grams at cathode for different amounts of time
2. Electrolysis of molten NaCl in a Downs cell is the major isolation step in the production of sodium metal. Assuming that 215 g of Na metal forms, a. How many moles of electrons are required? b. How many coulombs are required? C. How many amps will produce this amount in 9.50 h?