21.29 Consider the following voltaic cell: Voltmeter Fe Ni Salt bridge 1'M Fe2+ (a) In which direction do electrons flow in the external circuit? (b) In which half-cell does oxidation occur? (c) In which half-cell do electrons enter the cell? (d) At which electrode are electrons consumed? (e) Which electrode is negatively charged? (f) Which electrode decreases in mass during cell operation? (g) Suggest a solution for the cathode electrolyte. (h) Suggest a pair of ions for the salt bridge.

21.29 Consider the following voltaic cell: Voltmeter Fe Ni Salt bridge 1'M Fe2+ (a) In which direction do electrons flow in the external circuit? (b) In which half-cell does oxidation occur? (c) In which half-cell do electrons enter the cell? (d) At which electrode are electrons consumed? (e) Which electrode is negatively charged? (f) Which electrode decreases in mass during cell operation? (g) Suggest a solution for the cathode electrolyte. (h) Suggest a pair of ions for the salt bridge.

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

Consider a voltaic cell at 258C in which the following reaction takes place. 3 O2(g)+4NO(g)+2H2O= 4NO^-3(aq)+4H^+(aq) (a) Calculate Eº (b) Write the Nernst equation for the cell (c) Calculate E under the following conditions: [NO3¯ ] = 0.750M; PNO = 0.993 atm; Po2 = 0.515 atm; pH = 2.85
Please answer in full sentences
A voltaic cell using Cu/Cu²+ and Sn/Sn²+ half-cells is set up at standard conditions, and each compartment has a volume of 345 mL. The cell delivers 0.17 A for 31.5 h. (a) How many grams of Cu(s) are deposited? 9.7 (b) What is the [Cu²+ ] remaining? 0.56
Consider the following line notation: Cu(s)│Cu(NO3)2 (aq) (0.00678 M)║ Al(NO3)3 (aq) (0.00345M)│Al(s) Calculate E for this electrochemical cell set up ignoring activity coefficients. Recalculate E for the electrochemical cell with activity coefficients. (
Please Help me answer this, thank ue
An electroplating process uses 15.0 A to chemically corrode (dissolve) a copper anode. What is the corrosion rate of the anode in grams per hour?
5) For this problem refer to the electrochemical cell below a) Which electrode is the cathode and which is the anode? b) Is this cell electrolytic or galvanic? Explain. c) If the concentration of dissolved zinc ions were increased, how would this change the measured voltage? Volumeter so so; Znisi - Zntag) - 2e Cagl + 2e -Cuis)
I need help with all parts. Thanks
please help
Consider the reaction in a lead storage battery below. Which of the following statements is correct? PbO2(s) + Pb(s) + 2 H2SO:(aq) = 2 PBSO:(s) + 2 H2O(1) B) Pb2- is formed at the cathode during use of the battery. C) The mass of Pb decreases during recharging. E) The mass of PBSO4 remains constant during use and recharging of the battery.
a) Balance the following redox reaction in basic solution: H2O2(aq) + ClO2(aq) → ClO2-(aq) + O2(g) b) Sketch the voltaic cell for the redox reaction, labeling the direction for electron flow, the anode and cathode , and the species present in each half-cell. Show all the work please!
Fully label the unlabelled Galvanic cell below using the following information: Electrodes: Magnesium and Zinc Salt Bridge: KNO3 a- Identify the anode and cathode (and the solution each is in) b- Write the anode and cathode half-cell reactions c- Write the overall cell reaction d- Show the direction of e- flow e- Show the direction of ion flow in the salt bridge f- Predict which electrode will increase in mass and which electrode will decrease in mass. Explain your answer.