Based on the reduction potential, which of the following metal can serve as a sacrificial metal for the cathodicprotection of the chromium metal?nickelmagnesiumtinaluminumсopperMAY15山T6MacBook Air000D00 F4F7F8F9F6F5F1F2F3$&568923

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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...

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Complete and balance the following half-reaction in basic solution
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According to Standard reduction potentials table on page 164 (OLI), which of the following metals would reduce Sn (tin) from its solution? Sn+2 + 2e Sn O Au (gold) O Fe (Iron) O Pb (lead) O Cu (copper)
Balance the following reaction by the electron ion method.
Balance the following redox reaction in acidic solution.
Standard Reduction Potentials at 25 °C Half-reaction. Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e →→Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Aut 2Au + Au³+ Will Au* disproportionate in aqueous solution? To justify your answer, what is the standard cell voltage for the disproportionation reaction?
1. Consider the following standard reduction potentials in acid solution: E°(V) -1.66 +0.07 +0.14 Fe³+ + e +0.77 The strongest reducing agent among those shown above is Hint: If answer is with charge, type this way: X2+ Al³+ + 3e → Al(s) AgBr(s) + e → Ag(s) + Brā Sn4+ + 2e → + 2e → Sn²+ Fe²+
Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Sn metal is put into a 1M aqueous Co2* solution. If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. >
19 eq eq 2re 2req 2req Its 2req ots 2req #3 Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Cu2+ (aq) + Fe(s)→ Cu(s) + Fe²+ (aq) E Cu2+ (aq) + 2e Fe2+ (aq) +2e AG = kj K for this reaction would be Submit Answer $ 4 R → Cu(s) Ee red → Fe(s) Fred % 5 = 0.337 V Retry Entire Group 9 more group attempts remaining T = -0.440 V e than one. Cengage Learning Cengage Technical Support 6 MacBook Pro Y 887 & U * 8 1 ( 9 ) 0 (Pre- Email Ins 0 P
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.
Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)
13.71 Round your answers to 6 decimal places

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Based on the reduction potential, which of the following metal can serve as a sacrificial metal for the cathodic protection of the chromium metal? nickel magnesium tin aluminum сopper MAY 15 山T6 MacBook Air 000 D00 F4 F7 F8 F9 F6 F5 F1 F2 F3 $ & 5 6 8 9 23