MISSED THIS? Watch KCV: Cell Potential and Concentration; Read Section 20.6. You can click on the Review link to accessthe section in your e Text.2+2+A voltaic cell consists of a Pb/Pb² half-cell and a Cu/Cu²+half-cell at 25 °C. The initial concentrations of Pb²+are 0.0500 M and 1.50 M, respectively.and Cu²+▼Part C2+What is the concentration of Pb²+ when the cell potential falls to 0.370 V ?Express your answers using three significant figures.► View Available Hint(s)2+[Pb²+] =SubmitIVF ΑΣΦPrevious AnswersX Incorrect; Try Again; 4 attempts remaining?M

[Pb2+] = 0.0500 M[Cu2+] = 1.50 Mn = 2 electron transferEoCu2+/Cu = 0.34 VEoPb2+/Pb = -0.126 VEcell =…

MISSED THIS? Watch KCV: Cell Potential and Concentration ; Read Section 20.6. You can click on the Review link to access the section in your e Text. A voltaic cell consists of a Pb/Pb²+ half-cell and a Cu/Cu²+ half-cell at 25 °C. The initial concentrations of Pb²+ and Cu²+ are 0.0500 M and 1.50 M, respectively. Part C What is the concentration of Pb²+ when the cell potential falls to 0.370 V ? Express your answers using three significant figures. ▸ View Available Hint(s) [Pb²+] = Submit 195] ΑΣΦ Previous Answers B ? M

MISSED THIS? Watch KCV: Cell Potential and Concentration ; Read Section 20.6. You can click on the Review link to access the section in your e Text. A voltaic cell consists of a Pb/Pb²+ half-cell and a Cu/Cu²+ half-cell at 25 °C. The initial concentrations of Pb²+ and Cu²+ are 0.0500 M and 1.50 M, respectively. Part C What is the concentration of Pb²+ when the cell potential falls to 0.370 V ? Express your answers using three significant figures. ▸ View Available Hint(s) [Pb²+] = Submit 195] ΑΣΦ Previous Answers B ? 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...

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You have two beakers. One beaker contains 1 M Hg²* and 1 M Hg22*. The second beaker contains 1 M Fe2* and 1 M Fe*. All metals are present as their soluble nitrate salts. Design and draw a galvanic cell using these solutions (if you need other materials to complete the cell, you may add them in – state what they are needed for). Show the direction the electrons move (and where they move) and label the cathode and anode. Give the net ionic equation for the spontaneous reaction taking place in this galvanic cell. What would E°sell be?
For a voltaic cell based on the reaction below, which statement is correct?Zn(s)+2H+(aq)→Zn2+(aq)+H2(g) a. Zn2+(aq) is oxidized at the anode. b. H+(aq) is reduced at the cathode. c. Zn2+(aq) is reduced at the anode. d. H2(g) is the oxidizing agent.
For the functioning of a voltaic cell using the reaction below, which statement is true?Ni(s)+2AgNO3(aq)→Ni(NO3)2(aq)+2Ag(s) a. Nitrate ions will diffuse toward the anode side. b. Nickel(II) ions will diffuse toward the cathode. c. Nickel(II) ions will diffuse toward the anode. d. Silver will precipitate on the anode side.
Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. 2 Ag*(aq) + Pb(s) → 2 Ag(s) + Pb²+(aq) b. Ni?+ (aq) + Mg(s) → Ni(s) + Mg²*(aq) c. Calculate E°cell values for (a) and (b). Show your work. d. Show the cell notations for (a) and (b)
Explain the process of electrolysis using the diagram below. Where does oxidation occur? Where does reduction occur? Describe the direction of the flow of electrons. How is this electrolytic cell different from a voltaic cell? Note: The symbol Me stands for a metal. Show all work and answer in complete sentences.
1.Read the statements. I. The cell needs continuous supply of hydrogen to operate. II. The cell is used in some cars. III. Water is a byproduct of the redox reaction. What type of voltaic cell is described here? lead-acid cells dry cells wet cells fuel cells
What happens at the anode in the voltaic cell? Cathode?
2.What is the standard cell potential of an electrochemical cell? A.the sum of standard electrode potential of the two half-cells B.the standard electrode potential of the anode, relative to a hydrogen cell C.the difference between the standard electrode potential of the two half-cells D.the standard electrode potential of the cathode, relative to a hydrogen cell
What statement is true for a galvanic cell? a. Electrons move from the reduction to the oxidation half-reaction. b. The salt bridge is used to transport electrons. c. Oxidation takes place at the anode. d. The standard cell potential is negative.
A student makes a voltaic cell but forgets to include the salt bridge, then uses a voltmeter to measure the voltage. What will happen? The reaction will proceed much more slowly. The student may possibly suffer from an electric shock. Nothing- no reaction is possible. The reaction will happen only in one half-cell.
Cu
13. Compare and contrast an electrolytic cell with a voltaic cell. Provide one example where both are present in daily life. Electrolytic Cell Differences Similarities Voltaic Cell Differences h