Based on the half-reactions and their respective standard reduction potentials below, which addition toan aqueous solution containing Fe3+ will result in a reduction of Fe3+ ?02(g) + 4 H+ +4 e- → 2 H2O(I1)1.23 VFe3+(aq) + e- → Fe2+(aq)0.77 VCu2+(aq) + 2 e- → Cu(s)0.34 V2 H+(аq) + 2 е-> Н2(g)0.00 VNi2+(aq) + + 2 e- → Ni(s)-0.26 VFe2+(aq) + 2 e- → Fe(s)-0.45 VWater (H2O (I) )hydrogen gasoxygen gasaqueous copper(II) acetateNone

Redox reactions are those in which oxidation and reduction processes occur at the same time. It…

Based on the half-reactions and their respective standard reduction potentials below, which addition to an aqueous solution containing Fe3+ will result in a reduction of Fe3+ ? 02(g) + 4 H+ +4 e- → 2 H2O(1) 1.23 V Fe3+(aq) + e- → Fe2+(aq) 0.77 V Cu2+(aq) + 2 e-→ Cu(s) 0.34 V 2 H+{аg) + 2 е- H2(g) 0.00 V Ni2+(aq) + + 2 e- → Ni(s) -0.26 V Fe2+(aq) + 2 e- → Fe(s -0.45 V O Water (H2O (I) ) O hydrogen gas O oxygen gas aqueous copper(II) acetate None

Based on the half-reactions and their respective standard reduction potentials below, which addition to an aqueous solution containing Fe3+ will result in a reduction of Fe3+ ? 02(g) + 4 H+ +4 e- → 2 H2O(1) 1.23 V Fe3+(aq) + e- → Fe2+(aq) 0.77 V Cu2+(aq) + 2 e-→ Cu(s) 0.34 V 2 H+{аg) + 2 е- H2(g) 0.00 V Ni2+(aq) + + 2 e- → Ni(s) -0.26 V Fe2+(aq) + 2 e- → Fe(s -0.45 V O Water (H2O (I) ) O hydrogen gas O oxygen gas aqueous copper(II) acetate None

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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eq req *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: 2H+ (aq) + Fe(s)→ H₂ (s) + Fe²+ (aq) H₂ (8) E Fe(s) E E 2H+ (aq) +2e Fe2+ (aq) +2e -> AGO kj K for this reaction would be Submit Answer $ 4 R % 5 Retry Entire Group 9 more group attempts remaining = 0.000 V red=-0.440 V T red e than one. Cengage Learning Cengage Technical Support 6 MacBook Pro Y & U * 00 8 1 ( 9 K 0 0 Previous Email Instructo P
7. Please answer the following questions. (a) Given the following reduction potentials Cd (OH)2 (s) + 2e → Cd (s) + 2 OH (aq) Eºred = -0.76 V NIO(OH) (s) + H₂O (1) + e → Ni(OH)2 (aq) + OH (aq) Eºred = +0.49 V Calculate the standard emf of the nickel-cadmium (nicad) rechargeable battery. *hint: the reaction for the discharge of nicad battery is: Cd (s) + 2 NIO(OH) (s) + 2 H₂O (1)→ 2Ni(OH)2 (aq) + Cd(OH)2 (s) (b) A typical nicad voltaic cell generates an emf of +1.30 V. Why is there a difference between this value and the one you calculated in part (b)? (c) Calculate the equilibrium constant for the overall nicad reaction based on this typical emf value.
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. 2Cr(OH)3 (s) +100H¯ (aq) +3Zn²+ (aq) → 2CrO²¯ (aq) +8H₂O (1) + 3 Zn (s) 0 x10 X
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Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: Cd2+ (aq) + Zn(s)→→→→→→ Cd(s) + Zn²+ (aq) Answer: kJ K for this reaction would be than one.
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Cl₂ (g) + 2 e →2 Cl(aq) O2(g) + 4 H3O+ (aq) + 4 e 6 H₂O(1) 1.360 1.229 2 H2O(l) + 2e Al3+ (aq) + 3 e → Al (s) H2(g) + 2 OH(aq) -0.828 -1.660 A 0.114 M neutral aqueous AlCl3 solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential?
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Consider the following standard reduction potentials: Zn2*(aq) + 2 e → Zn(s) E° = -0.76 V Mg2*(aq) + 2 e → Mg(s) E° = -2.37 V Ag*(aq) + e → Ag(s) E° = +0.80 V Which is the strongest oxidizing agent? Mg2*(aq) Zn2*(aq) Ag*(aq) 5:08 PM 90°F Partly sunny P Type here to search 8/6/2021
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.