LEARNING CHECK 4.2Competencies8. define reduction potential, oxidation potential, and cell potential9. describe the standard hydrogen electrode10. calculate the standard cell potential11. relate the value of the cell potential to the feasibility of using thecell to generate an electric current1. Compare the relative oxidizing and reducing strengths of the substances listed in theTable of Reduction Potentials.2. Determine the cell potentials for the following reactions:a) Agʻ + Mg →Ag + Mgb) AgCl + Fe →Ag+ Fe" + Ci3. Which of the following reactions have the greater tendency to attain equilibrium?A. Co" + Ni →Co + Ni",B. Sn+Cu4. Evaluate the standard cell potential of each of the following cells, and determinewhether the cell is galvanic or electrolytic.lagCu+ Snlaga) Au+ Fe+→Au(s) + 4 CI + Fe*b) K +H,0-O + H* + K5. The alkaline battery is the most common primary non-rechargeable batterynowadays. Its anode consists of powdered zinc metal mixed with gel that is incontact with concentrated KOH solution which is why it is called alkaline battery.The cathode is a mixture MnO2(s) and graphite. The mixture is separated from the

8.) Reduction potential refer to the tendency of a chemical species to gain electrons and exit in…

LEARNING CHECK 4.2 Competencies 8. define reduction potential, oxidation potential, and cell potential 9. describe the standard hydrogen electrode 10. calculate the standard cell potential 11. relate the value of the cell potential to the feasibility of using the cell to generate an electric current

LEARNING CHECK 4.2 Competencies 8. define reduction potential, oxidation potential, and cell potential 9. describe the standard hydrogen electrode 10. calculate the standard cell potential 11. relate the value of the cell potential to the feasibility of using the cell to generate an electric current

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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O ELECTROCHEMISTRY Designing a galvanic cell from two half-reactions A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction 2+ Fe (aq) Ed=+0.771 V %3D 3+ red Fe"(aq)+e Cro (aq)+4 H,O(1)+3e Cr(OH),(s)+5OH (aq) -0.13 V Ered nswer the following questions about this cell. Jrite a balanced quation for the alf-reaction that appens at the athode. rite a balanced uation for the If-reaction that ppens at the ode. ite a balanced uation for the erall reaction
i. Doubling the size of the Fe (m) bar will INCREASE DECREASE NOT CHANGE (circle one) the voltage of the cell. j. Doubling the concentration of Ag*(aq) will INCREASE DECREASE NOT CHANGE (circle one) the voltage of the cell. k. Adding 1.0 M NaCl solution to the beaker in the right will INCREASE DECREASE NOT CHANGE (circle one) the voltage of the cell.
2)
Number 2
Consider the cell described below. Al | Al³+ (1.00 M) || Pb²+ (1.00 M) | Pb Calculate the cell potential after the reaction has operated long enough for the [A13+] to have changed by 0.46 mol/L. (Assume T= 25°C.) V Need Help? Read It Supporting Materials Periodic Table Watch It Constants & Factors Supplemental Data
Examine the following information below for a electolytic cell and answer the following questions: Procedure: Procedure: Constructing an Electrolytic Cell (convert energy to ions) 1. Obtain a 6-volt battery, electrodes, and plastic sample cup necessary to build an electrolytic cell like that shown in figure 2 below. Obtain a pH meter and set it to begin collecting data. 2. Weigh 2.0 g of solid KI. Record the mass. Transfer the solid to an Erlenmeyer flask. 3. Add 100 mL of deionized water (measure using a graduated cylinder) to the flask and swirl it until a homogeneous solution is formed. Measure and record the initial pH of this solution. 4. Transfer the 100 mL of KI solution from the Erlenmeyer flask to the plastic sample cup. Place the lid containing the electrodes on top of the sample cup. Attach wires from the batter to the electrodes. Note and record your start time. 5. Observe the electrolysis for several minutes. Record your observations at…
Solve it asap... Standard potential can be found in Google or any book
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ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.78 minutes for a current of 1.35 A to plate 0.0808 g of metal from a solution containing M2(SO4)3. Input values only with 2 decimal places. Do not include the unit. Round your answer to 2 decimal places. Add your answer
show-all-working-explaining-detailly-each-step Answer should be typewritten with a computer keyboard.
Research and write a report on the use of zinc as a “sacrificial anode” to minimize the corrosion of iron and steel such as on ships. Use the standard electrode potentials given in question 2 above to predict the cell emf and overall equation for the reaction that would occur in standard conditions between zinc and iron. With ocean-going ships, however, what is the solution in which the two metals are immersed? Is this solution always at an exact concentration of 1 mol dm-3? And in what ways does this real-life situation differ from the standard condition of 25oC / 298K
INTERACTIVE EXAMPLE Electroplating How long will it take to plate out 4.2 g Ni from aqueous Ni2+ with a current of 112.3 A? HOW DO WE GET THERE? What is the quantity of charge carried by these electrons (in C)?