Use the References to access important values if needed for this question The free energy of an electrochemical cell is given by the equation: AG=-nFE Where: AG=Gibbs Free Energy change n = moles of electrons F = Faraday's constant. Ecell voltage NOTE: Write AG as dG (with no spaces) for the answers below. In order to solve for the Faraday's constant, F. you must multiply both sides of the equation by the same expression: AG X x=- =-nFE x The resulting equation is: F =

Use the References to access important values if needed for this question The free energy of an electrochemical cell is given by the equation: AG=-nFE Where: AG=Gibbs Free Energy change n = moles of electrons F = Faraday's constant. Ecell voltage NOTE: Write AG as dG (with no spaces) for the answers below. In order to solve for the Faraday's constant, F. you must multiply both sides of the equation by the same expression: AG X x=- =-nFE x The resulting equation is: F =

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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Consider a galvanic cell for which the anode reaction isPb(s) → Pb+2 (0.010 M) + 2e- , E= -0.1263 VAnd the cathode reaction isVO2+ (0.10 M) + 2H+ (0.10 M) + e- → V3+ (1.0×10-5 M) + H2O (l) , E =?The measured cell potential is 0.640 V.a) Calculate the E cell for the cathode.b) Calculate the equilibrium constant for the overall reaction. c)Calculate ΔG for this reaction in kJ d) Determine the pH of this cell
Which of the following are standard conditions for an electrochemical cell? 1. Solutes in aqueous solution have a concentration of 1.0 M. 2. Gaseous reactants or products have a pressure of 1 bar. 3. Solids are present in quantities of 1 mole.
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Enter electrons as e". Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Ag*(aq) + Fe2*(aq) → Ag(s) + Fe³*(aq) The anode reaction is: The cathode reaction is: In the external circuit, electrons migrate the Fe2*|Fe3+ electrode the Ag|Ag* electrode. In the salt bridge, anions migrate v the Fe2"|Fe3+ compartment v the Ag|Ag" compartment.
A student made measurements on some electrochemical cells and calculated three quantities: . The standard reaction free energy AGO. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 2. calculated quantities (Check the box next to any that are wrong.) cell n AGⓇ ΔG K Eº - 32 A 2 А -178. kJ/mol 6.54 × 10 -0.92 V B 179. kJ/mol 2.29 X 10 -0.93 V с 2 127. kJ/mol 1.78 × 10²2 0.66 V 31 X ?
How many hours are required to produce 795 grams of lead from molten lead(II) chloride (PbCl2, 278.1 g/mol) if the current used is 116 amps? Faraday's constant is 96,485 C/mol e-. Write your answer with 3 significant digits.
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The free energy change for the following reaction at 25 °C, when Sn²+ 2+ [Zn²+] = 0.00776 M, is -133 kJ: [Sn²+] = 1.11 M and Sn²+ (1.11 M) + Zn(s) → Sn(s) + Zn²+ AG = -133 kJ What is the cell potential for the reaction as written under these conditions? Ecell V Sn(s) + Zn²+ (0.00776 M) Would this reaction be spontaneous in the forward or the reverse direction? O forward direction O reverse direction
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A certain metal M forms a soluble nitrate salt MNO,. Suppose the left half cell of a galvanic cell apparatus is filled with a 3.50 M solution of MNO, and the right half cell with a 17.5 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. left x10 Which electrode will be positive? right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
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