A student does an experiment to determine the molar solubility of lead() iodide. He constructs a voltaic cell at 298 K consisting of 0.883 M lead nitrate solution and a lead electrode in the cathode compartment, and a saturated lead iodide solution and a lead electrode in the anode compartment. If the cell potential is measured to be 8.30x102 V, what is the value of Ksp for lead iodide at 298 K based on this experiment? Ksp for Pbl₂=

A student does an experiment to determine the molar solubility of lead() iodide. He constructs a voltaic cell at 298 K consisting of 0.883 M lead nitrate solution and a lead electrode in the cathode compartment, and a saturated lead iodide solution and a lead electrode in the anode compartment. If the cell potential is measured to be 8.30x102 V, what is the value of Ksp for lead iodide at 298 K based on this experiment? Ksp for Pbl₂=

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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I have solved this equation and seen solutions to it. However, I keep seeing Pb2+ squared in the Nernst Equation (for Q) for the calcuation of the second part of this question. I do not understand why Pb2+ is squared. Can you explain that to me? Thank you.
Pb(s) Determine which of the following statements about the cell shown are True or False. True The standard cell potential, o, equals 0.93 V. True As the reaction proceeds, the concentration of the silver ions decreases. False Cations move to the lead half-cell. True The mass of the silver electrode is increasing. True The silver half-cell is the cathode. False The cell, as represented by the line notation, is a voltaic cell. True True The lead electrode is the anode. Electrons are spontaneously produced in the silver half-cell. salt bridge Ag(s) Pb+2 So Pb2+2e → Pb(s) AS NO3 E--0.13V Ag + le → Ag(s) E° - +0.80V Pb(s) Pb2+ (1M) || Ag+ (1M) | Ag(s)
A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl₂ for 15.5 h. What mass of Mg is produced? g
A chemist designs a galvanic cell from the following two half-reactions Ered = +0.96 V NO3(aq) + 4H+ (aq) + 3e¯ → NO(g) + 2H₂O (1) Ered +0.153 V Cu²+ (aq) + e¯ → Cut (aq) The standard cell potential for this galvanic cell is [Select] The standard free energy for this galvanic cell is AG [Select] The equilibrium constant (K) for this galvanic cell is [Select] = V.
A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M1.0 M tin(IV) ion and 1.0 M1.0 M tin(II) ion, and another inert platinum electrode in a solution containing 1.0 M1.0 M cerium(IV) ion and 1.0 M1.0 M cerium(III) ion, connected by a salt bridge. Calculate the standard potential for this cell at 25°C25°C. Standard reduction potentials can be found in the standard reduction potentials table.
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A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn (aq)+Ba (s) Sn (s)+ Ba" (aq) 2+ Suppose the cell is prepared with 4.24 M Sn 2+ in the other. in one half-cell and 2.000 M Ba' Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
A student constructed a voltaic cell by combining Sn/Sn2+ and Zn/Zn2+ two half cells and measured a cell potential of 0.620 V. He then constructed a voltaic cell by combining Sn/Sn2+ and Ni/Ni2+ two half cells and measured a cell potential of 0.140 V. It is seen that the tin metal precipitated out of the solution in each above cell. Except for the reduction potential of Zn which is known as -0.763V, the reduction potentials of all the other two electrodes are unknown. a. Calculate the reduction potential of Sn2+ (aq)+ 2e- ---> Sn(s). b. Calculate the reduction potential of Ni2+(aq)+2e- ----> Ni(s) c. Write the cell reaction for the cell of Sn/Sn2+ and Zn/Zn2+
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