Calculate \( K_c \) for the system \( \text{Ni}^{2+} + \text{Co} \rightleftharpoons \text{Ni} + \text{Co}^{2+} \). Assume \( T = 298 \, \text{K} \).\[\begin{array}{|c|l|}\hlineE^\circ \, (\text{Volts}) & \text{Half-Cell Reaction} \\\hline-0.25 & \text{Ni}^{2+} (aq) + 2e^- \rightarrow \text{Ni} (s) \\-0.28 & \text{Co}^{2+} (aq) + 2e^- \rightarrow \text{Co} (s) \\\hline\end{array}\]The table lists the standard reduction potentials (\( E^\circ \)) and the corresponding half-cell reactions for nickel and cobalt.

first we will calculate the Electrode potential of the cell here we can see Ni+2 is reduced to Ni…

Answered: Calculate K. for the system Ni2+ + Co S…

Calculate K. for the system Ni2+ + Co S Ni + Co2+. Assume T = 298 K. E° (Volts) Half-Cell Reaction Ni (ag) +2e Co2" (aq) + 2e -0.25 Ni(s) -0.28 Co(s)

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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10.)
a) Consider the sparingly soluble salt silver bromide. Write a balanced chemical equation showing the dissolution of silver bromide. b) Given the following information, provide the net reaction for the spontaneous reaction and determine the cell potential under standard conditions that would occur from these two half-reactions: Ag+(aq) + e- ⟶⟶ Ag(s) E°red = 0.80 V AgBr(s) + e- ⟶⟶ Ag(s) + Br-(aq) E°red = 0.07 V c) Calculate the equilibrium constant at 283 K (10.° C) for the spontaneous redox reaction you wrote in part b. d) Using only the information provided in this problem, calculate the solubility product constant of silver bromide at 10. °C. e) Is the dissolution of silver bromide at 10. °C thermodynamically favorable? Justify your response by determining ΔΔG°rxn at 10. °C, using only the information provided or determined in this problem.
Consider a galvanic cell at T = 298K. F = 96 485C. At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+] = 2M. Consider the half-reactions below: Ca2+(aq) + 2e- → Ca(s) E0red = - 2.76 V HfO2+(aq) + 2H+(aq) + 4e- → Hf(s) + H2O(l) E0red = -1.72 V d. Express and calculate Q (at t0) e. Express and calculate K. f. What value do you expect for Ecell at this point? Why? g. Find Ecell (at t0)
What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0360 V and n = 2?(F = 96,500 J/(V･mol), R = 8.314 J/(mol･K))
Paragraph Font Given the reaction and the half-cell potentials: Zn(s) + Pb2+(aq) → Zn2+(aq) + Pb(s) Ecell oxidation= -0.763V Ecell reduction = -0.126V Determine the half-cell reactions, anode and cathode, cell potential and cell diagram.
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e- 2 Br-(aq) 1.08 NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O(l) 0.96 2 Hg2+(aq) + 2 e- Hg22+(aq) 0.920 Hg2+(aq) + 2 e- Hg(l) 0.855 Ag+(aq) + e- Ag(s) 0.799 Hg22+(aq) + 2 e- 2 Hg(l) 0.789 Fe3+(aq) + e- Fe2+(aq) 0.771 I2(s) + 2 e- 2 I-(aq) 0.535 Fe(CN)63-(aq) + e- Fe(CN)64-(aq) 0.48 Cu2+(aq) + 2 e- Cu(s) 0.337 Cu2+(aq) + e- Cu+(aq) 0.153 S(s) + 2 H+(aq) + 2 e- H2S(aq) 0.14 2 H+(aq) + 2 e- H2(g) 0.0000 Pb2+(aq) + 2 e- Pb(s) -0.126 Sn2+(aq) + 2 e- Sn(s) -0.14 Ni2+(aq) + 2 e- Ni(s) -0.25 Co2+(aq) + 2 e- Co(s)…
Consider a galvanic cell at T = 298K. F = 96 485C. At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+] = 2M. Consider the half-reactions below: Ca2+(aq) + 2e- → Ca(s) E0red = - 2.76 V HfO2+(aq) + 2H+(aq) + 4e- → Hf(s) + H2O(l) E0red = -1.72 V a. Find the general reaction, E0cell, and identify the cathode and the anode. Indicate the direction of the flow of electrons (from which solid plate to the other solid plate). b. Write the line notation for this cell. c. Find ΔG0. *d. Express and calculate Q (at t0) e. Express and calculate K. f. What value do you expect for Ecell at this point? Why? g. Find Ecell (at t0) After a certain period of time (t1), the H+ concentration is one-fifth of its initial concentration. *h. Do the RICE and find the concentrations of all species at t1 i. Find the pH at t1 in two…
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Use the Nernst equation to calculate the cell potential at 298K. Cu(s) + PtCl ² (aq) (0.10M) → Cu²+ (aq) (0.20 M) + PtCl 4² (aq) (0.10M) + 2Cl(aq) (0.40M) • Ered Cu²+ (aq)/Cu(s) = +0.34 V • Eºred PtCl 6² (aq)/ PtCl4²(aq) + 2Cl¯ Oxidation: Cu(s)→→ Cu²+ (aq) + 2 e 2- Reduction: PtCl6² (aq) + 2 e → PtCl 4² (aq) + 2Cl(a (aq) √(aq) = ₁ = +0.68 V Ex = -0.34 V Eº = +0.68 V red
Calculate the Ecell Value at 298 K for the cell based on the reaction: Cu(s)+2Ag*(aq) Cu²+(aq) +2Ag(s) where [Ag*] = 0.00375 M and [Cu2+] = 8.25×104 M. The standard reduction potentials are shown below: Ag"(aq) +e → Ag(s) E° : 0.7996 V Cu²+ (aq) + 2e¯ → Cu(s) E° = 0.3419 V 3rd attempt Feedback Ecell= 0.47713 V
3) Use half cell potentials to determine if each reaction occur spontaneous in the direction written (yes/no). a) Ca¹2(aq) + Zn(s) - Ca(s) + Zn¹²(aq) b) Au*³(aq) + Ag(s) - Au(s) + Ag (aq) c) Co(s) + Pb (aq) - Co²(aq) + Pb(s) d) Pb(aq) + H₂S(g) -Pb¹2(aq) + S(s) ing if each metal will dissolve in 1M HCl.
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn/Zn2+ half-cell and an H2/H+ half-cell under the following conditions: [Zn2+ ] = 0.041 M [H+ ]= 1.2 M partial pressure of H2 = 0.52 atm. Calculate Ecell at 298 K (enter to 3 decimal places). Zn2+ (aq) + 2e Zn(s) E° = 0.76 V 2H+ (aq) + 2e H2(g) E° = 0.00 V