**Writing the Cell Diagram for the Given Electrochemical Cell**The diagram illustrates a galvanic (voltaic) cell, consisting of two half-cells connected by a salt bridge. The components of this electrochemical cell are detailed below:### Components:- **Left Half-Cell:** - **Electrode:** A platinum (Pt) electrode, used as an inert conductor. - **Solutions/Compounds:** - Potassium chloride (\(\text{KCl(aq)}\)) is the electrolyte. - Mercurous chloride (\(\text{Hg}_2\text{Cl}_2(s)\)) is a solid. - Elemental mercury (\(\text{Hg(l)}\)), which is in liquid form.- **Right Half-Cell:** - **Electrode:** Zinc (\(\text{Zn}\)) metal. - **Solution:** Zinc chloride (\(\text{ZnCl}_2(aq)\)) serving as the electrolyte.### Connections:- An external circuit connects the two electrodes shown by the wires leading from the \(-\) terminal (left) to the \(+\) terminal (right) through a voltmeter (V), allowing electron flow.- A salt bridge is included between the two solutions to maintain electrical neutrality by allowing the migration of ions.### Cell Diagram:The cell diagram, representing the reaction occurring in the galvanic cell, is written as follows:\[\text{Pt} | \text{Hg}_2\text{Cl}_2(\text{s}) | \text{Hg}(\text{l}) || \text{ZnCl}_2(\text{aq}) | \text{Zn}\]**Explanation:**- The single vertical lines (\(|\)) represent phase boundaries. - The double vertical line (\(||\)) signifies the salt bridge separating the two half-cells.- The left side denotes the anode side (oxidation occurs, \(-\) electrode).- The right side denotes the cathode side (reduction occurs, \(+\) electrode).This cell generates electrical energy through a spontaneous redox reaction, which can be measured with the voltmeter in the circuit. Using a diagrammatic representation such as this is crucial for visualizing the components and reactions of galvanic cells in electrochemistry.

Anode reaction - Hg(l) ------> Hg2+(aq) + 2e Cathode reaction - Zn2+(aq) + 2e -----> Zn(s)…

Answered: Write the cell diagram for the…

Science

Chemistry

Write the cell diagram for the following cell. + V KCI(aq) Hg,Cl2(s) Pt Hg(1) ZnCl2(aq) uz

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 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)
Consider the cell below at standard conditions: Zn(s) | Zn 2+ (aq) || Fe 2+ (aq) | Fe(s)Calculate the value of ΔG° for the reaction that occurs if the value of E° cell = 0.32 V for this cell.
Can you break down the problem attached?
If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2 is 1.00 atm, calculate the cell potential at 25.0°C.
Consider the voltaic cell diagrammed below: Pb (s)| Pb²+ (aq)l| H2 (g)| H* (aq) | Pt (s) a) Write the balanced chemical equation that occurs in the voltaic cell depicted in the diagram. b) If the concentration of Pb2+ in this cell is 0.035 M and the pH is 1.60, what pressure of H2 (g) would keep the cell reaction in equilibrium?
Questions 20 and 21 refer to the following information. Galvanic Cell Cell Diagram E°cell (Volts) Mg | Mg2(1.0 M) || Pb*2(1.0 M) | Pb 1 2.24 Zn | Zn(1.0 M) || Pb*2(1.0 M) | Pb 2 0.63 Mg | Mg*(1.0 M) || Zn*2(1.0 M) | Zn 3 The chemical reaction occurring in first galvanic cell is: Mg + Pb*2 → Mg+2 + Pb 21. If the concentration of Mg+2 is changed from 1.0 M to 3.0 M in the galvanic cells above, what will happen to the observed cell voltages in galvanic cells 1 and 3? (A) The voltage in both galvanic cells 1 and 3 will increase. (B) The voltage will decrease in both galvanic cells 1 and 3. (C) The voltage in galvanic cell 1 will increase and will decrease in galvanic cell 3 (D) The voltage in galvanic cell 3 will increase and will decrease in galvanic cell 1. 22. Consider a voltaic cell based on these half-cells. Ag (aq) +e → Ag/s) Cd (aq) + 2e → Cd¢s) E* = +0.80 V E = -0.40 V Identify the anode and give the voltage of this cell under standard conditions. (A) Ag; Ecell = 0.40 V (B) Ag;…
Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=