Al(s) + 3 Ag*(aq) Al3*(aq) +3 Ag(s)A voltaic cell utilizes the reaction above. What is the effect on the cell potential of each of thefollowing changes?a. Water is added to the anodec. Solid AgNO, is added to thecathode half-cell and dissolved.half-cell, diluting the solution.d. HCl is added to the Ag(NO3)solution, precipitating some of theAg* as AgCl.b. The size of the aluminumelectrode is increased.nYoninine

ECell = Ecathode - Eanode = Ereduction - Eoxidation Thus we have to 1st identify the cathode…

Al(s) + 3 Ag*(aq) Al*(aq) + 3 A -> A voltaic cell utilizes the reaction above. What is the effect c following changes? a. Water is added to the anode half-cell, diluting the solution. b. The size of the aluminum electrode is increased. Yor

Al(s) + 3 Ag(aq) Al(aq) + 3 A -> A voltaic cell utilizes the reaction above. What is the effect c following changes? a. Water is added to the anode half-cell, diluting the solution. b. The size of the aluminum electrode is increased. Yor

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

A galvanic cell runs for 1 minute with a current of 0.20 A. How much charge passed through the cell in that time? (F = 96,500 C/mol)
2. For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M)
Predict the potential for the following voltaic cell at 25 C:Cu(s)|CuSO4(1.29 M)||AgNO3(0.7 M)|Ag(s)
2.Write a balanced cell reaction. Include the phases of all species in the chemical equation.
Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.500 M and the concentration of the ion at the cathode is 1.50 M. Use the standard reduction potentials from Appendix L in our textbook.
22. The diagram below represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell? Al(s))Al³*(1.0 M)||Cu²*(1.0 M)|Cu(s) a. Al(s) + Cu (ag)→ Al** (aq) + Cu(s) b. 2H,0) + 3A1*(aq) + 2Cu(s) → 2A1(s) + 3Cu?*(aq) + 4H*(aq) + 0,(g) c. 2Al(s) + 3Cu?*(aq) → 3AI** (aq) + 2Cu(s) d. Al*(aq) + Cu(s) → Al(s) + Cu?*(aq) e. 3A* (aq) + 2Cu(s) → 2Al(s) + 3Cu²*(aq)
H11. Consider the voltaic cell H+ (aq, ?? M) H₂(g, 1 atm)||Cu(s) Cu²+ (aq. 0.1 M). Ecell for this cell at 25 C was +0.360V. What was the pH of the anode solution? A. 0 ABCDE B. C. D. E. 0.89 3.2 7.0 11.7
Using a table of standard electrode potentials, decide which of the following statements is completely true. Multiple Choice H* can oxidize Fe, and Ni can reduce Brz. Ni2" can oxidize Cu?", ond Fo2" can reduce H". O Cu2" can oxidize H2, and Fe can reduce Mn2". Br2 can oxidize Ni, and H2 can reduce Mn2 Fe" can oxidize H2, and Fe" can reduce Au".
I couldnt find the value for b and c on the table, so I'm not sure why the correct answer was C) Pb . can someone explain why. I want to know what to do during a test what to do when i cant find the values for a specific element on the table?
#26