Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co²+ (aq) + Cd(s) → Co(s) + Cd²+ (aq) Co2+ (aq) + 2e →Co(s) = -0.280 V Cd2+ (aq) +2e → Cd(s) F = -0.403 V red red Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be Retry Entire Submit Answer 9 more group attempts remaining than zero. greater

Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co²+ (aq) + Cd(s) → Co(s) + Cd²+ (aq) Co2+ (aq) + 2e →Co(s) = -0.280 V Cd2+ (aq) +2e → Cd(s) F = -0.403 V red red Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be Retry Entire Submit Answer 9 more group attempts remaining than zero. greater

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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Use standard reduction potentials to calculate the equilibrium constant for the reaction: I₂ (s) + 2Fe²+ (aq). → 21¯ (s) + 2Fe³+ (aq) 0.535 V, E³+ /Fe²+ From the table of standard reduction potentials: E Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be + than zero. 0.771 V
Using the standard reduction potentials listed in Appendix E in the textbook, calculate the equilibrium constant for each of the following reactions at 298 K. Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s)
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 31₂ (s) + 2Cr(s) → 61¯(s) + 2Cr³+ (aq) I₂ (s) + 2e¯ → 21¯ (s) Cr³+ r³+ (aq) + 3e¯ → Cr(s) E red kJ AGO = Eº = = 0.535 V red = -0.740 V
What is the value of the equilibrium constant at 25 oC for the reaction between the pair: Ag(s) and Mn2+(aq) to give Ag+(aq) and Mn(s) Use the reduction potential values for Ag+(aq) of +0.80 V and for Mn2+(aq) of -1.18 V
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2+ Cd²+ (aq) + Zn(s) → Cd(s) + Zn²+ (aq) AG⁰ = Cd2+ (aq) +2e → Cd(s) E red Zn²+ (aq) +2e → Zn(s) E red K for this reaction would be greater less = -0.403 V -0.763 V kJ than one.
Rank the following in increasing ability as oxidizing agents. The reduction potentials of all species are shown below. Cl, (g) + 2e → 2C1 (aq) E° = 1.3583 V Ag*(aq) + le Cu²+ (aq) + 2e¯ → Ag(s) E° = 0.7996 V → Cu(s) E° = 0.342 V Sn²+ (aq) + 2e → Sn(s) E° = - 0.136 V к"(ад) + 1е — → K(s) E° - 2.95 V 1st attempt
What is the equilibrium constant for the dissolution of copper (II) hydroxide: Cu(OH)₂ (s) Given the standard reduction potentials Cu(OH)₂ (aq) + e- → Cu (s) + OH¯ (aq) Cu²+ (aq) + e¯ →→ Cu (s) O 5.16 x 10^-9 O 1.63 x 10^3 O 1.93 x 10^8 O 6.12 x 10^-4 Cu²+ (aq) + OH¯ (aq) O 2.20 x 10^-20 EO = -0.15 V Eº = +0.34 V
Balance the following skeletal reaction in acidic solution. Be sure to include “1” in the blank if the coefficient is 1. Ag+(aq) +PbO(s) → PbO2(s) + Ag(s)
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2+ Co²+ (aq) + Zn(s) → Co(s) + Zn²+ (aq) red Co²+ (aq) + 2e → Co(s) Ee Zn²+ (aq) + 2e¯ → Zn(s) Ee red AGO K for this reaction would be kJ = -0.280 V -0.763 V than one.
Using standard reduction electrode potentials, calculate standard free-energy change at 25°C for the following reaction:3Cu(s) + 2NO3-(aq) + 8H+(aq) → 3Cu2+(aq) + 2NO(g) + 4H2O(l).
Just the last one. And use table if needed
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