**Educational Content: Galvanic Cell and Redox Reactions**A galvanic cell consists of a Ni/Ni²⁺ half-cell and a Co/Co²⁺ half-cell with initial concentrations:- \([Ni^{2+}]\) = 0.80M- \([Co^{2+}]\) = 0.20M - at 298.15 K.**Electrode Potentials:**\[\begin{array}{|c|c|}\hline\text{half-reaction} & E^\circ \text{(V)} \\\hlineNi^{2+}(aq) + 2e^- \rightarrow Ni(s) & -0.25 \\Co^{2+}(aq) + 2e^- \rightarrow Co(s) & -0.28 \\\hline\end{array}\]**Task 1: Write the balanced overall reaction that powers the cell.**[Your Answer Here]**Task 2: Calculate \(E_{cell}\) for the redox reaction.**Round to 2 decimal places.\[\boxed{\text{V}}\]**Task 3: Determine \([Ni^{2+}]\) when \(E_{cell}\) reaches 0.03V.**Round to 2 significant figures.\[\boxed{\text{M}}\]---**What happens at equilibrium?**1. **What is \(E_{cell}\) at equilibrium?** Round to 2 decimal places. \[ \boxed{\text{V}} \] 2. **\([Ni^{2+}]\) at equilibrium:** Round to 2 significant figures. \[ \boxed{\text{M}} \] 3. **\([Co^{2+}]\) at equilibrium:** Round to 2 significant figures. \[ \boxed{\text{M}} \]**Note:** For detailed explanations and step-by-step solutions, refer to the instructional content provided in the next section.---This content educates students on the construction and analysis of galvanic cells, focusing on half-reactions, electrode potentials, cell potential calculations, and equilibrium conditions.

The galvanic cell contains two half-cells: Ni/Ni2+ and Co/Co2+. Initial concentrations: [Ni2+] =…

A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28 Write the balanced overall reaction that powers the cell. Calculate Ecell for the redox reaction. (round to 2 decimal places) What is [Ni²+] when Ecell when reaches 0.03V? (round to 2 sig figs) V What happens at equilibrium? What is Ecell at equilibrium? [Ni²+] at equilibrium: [Co²+] at equilibrium: (round to 2 decimal places) (round to 2 sig figs) (round to 2 sig figs) M M M

A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28 Write the balanced overall reaction that powers the cell. Calculate Ecell for the redox reaction. (round to 2 decimal places) What is [Ni²+] when Ecell when reaches 0.03V? (round to 2 sig figs) V What happens at equilibrium? What is Ecell at equilibrium? [Ni²+] at equilibrium: [Co²+] at equilibrium: (round to 2 decimal places) (round to 2 sig figs) (round to 2 sig figs) M M M

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

Calculate the cell potential for the galvanic cell in which the reaction Al(s) + Au³(aq) Al³(aq) + Au(s) occurs at 25 °C, given that [A1³] = 0.00140 M and [Au³+] = 0.848 M. Refer to the table of standard reduction potentials. E=
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu2+ +2Al(s). (aq) + 2Al (s) 3Cu (s) + 2 Al³+ (aq) Suppose the cell is prepared with 5.70 M Cu2+ in one half-cell and 5.24 M A13+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ☐ x10 μ ロ・ロ
calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C Fe(s) | Fe3+ (aq, 0.0011M) || Fe3+(aq, 2.33M) | Fe(s)
Calculate the cell potential for a Galvanic cell based on the reaction described by the following unbalanced equation at 25 C (assume standard, acidic conditions). Cu(s) + MnO4-(aq) -> Cu2+(aq) + MnO2(s)
With explanation Find the standard change in free energy and the equilibrium constant for the galvanic cell resulting from the cell notation provided below. P(s)|Cr2+(aq),Cr3+(aq)|| Pb2+(aq)|Pb(s)
A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28
Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K. Cd2+(aq) + 2e– → Cd(s) E° = –0.403 V Pb2+(aq) + 2e– → Pb(s) E° = –0.126 V E°cell = ______________ Ecell = ______________
Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode. NO3- + H+ + Zn -> Zn2+ + NO2 + H2O
Write a balanced equation for the overall cell reaction in the following galvanic cell and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br (aq) | Br₂ (1) || Cl; (g) | Cl(aq) | Pt(s)
What is the balanced equation for the galvanic cell reaction expressed using the following shorthand notation? Mg (s) | Mg2+ (aq) || Cl2 (g) | Cl– (aq) | C (s)
An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a solution that is 2.5 M in KI and 0.046 M in I2. The other half-cell consists of magnesium metal immersed in a 0.37 M Mg2+ solution. Assume that the temperature is 25°C. (a) Which electrode is the anode and which is the cathode? anode: Pt|I2, I- O Mg²+|Mg cathode: O Pt|I2, I- Mg2+|Mg (b) What is the emf of the cell? 4.0 2.869 X V (c) What is the spontaneous cell reaction? chemPad OHelp Greek - Mg2+(aq)+21 (aq) Mg(s)+I2(aq) Mg(s)+l_2(aq)-->Mg^2+(aq)+2l^-(aq) Your answer appears to have inconsistent states-of-matter. (d) What is the equilibrium constant of the cell reaction? 2.42e98