A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell with [Ag*] = 5.00 × 10-2 M. Calculate the electromotive force of the cell at 25 °C. F= 96500 C/mol, R=8.314 J/mol.K The reduction potentials for the two half cells are: Ni2*(aq) + 2e →Ni(s) E° = -0.24 V Ag*(aq) + e¯ –Ag(s) E° = +0.8 V O a. 1.09 O b. 1.04 O c. 1.06 O d. 0.98 O e. 1.12

A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag/Ag half cell with [Ag] = 5.00 × 10-2 M. Calculate the electromotive force of the cell at 25 °C. F= 96500 C/mol, R=8.314 J/mol.K The reduction potentials for the two half cells are: Ni2(aq) + 2e →Ni(s) E° = -0.24 V Ag(aq) + e¯ –Ag(s) E° = +0.8 V O a. 1.09 O b. 1.04 O c. 1.06 O d. 0.98 O e. 1.12

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

X(s)|X5+ (0.94 M) || Mn O4 1 minus (1.10 M)|Mn O2(s)|H+ (0.51 M)The reduction potential for X5+ is 2.22 V. What is the potential of this non standard cell (in Volts)?
3. Standard reduction potentials are listed for reactions under standard conditions. Standard conditions are 1 M concentrations of ions, I atm (or I bar) partial pressures for gases, and a temperature of 298 K: In Part I, you were asked to compare your measured cell potential to a calculated standard cell potential. The cell potential you measured was for a galvanic cell you prepared using 0.10 M solutions of Pb2 and Cu, not 1.0 M solutions. Write out the balanced equation for this cell, then give the Nernst equation for this cell. From the Nernst equation, explain why the cell potential under these nonstandard conditions should be equal to the standard cell potential for this particular reaction. a.
Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3e – X(s) E° = -2.15 V Y3+ + 3 e –→ Y(s) E° = -0.29 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? E° 'cell V
describe the difference between Zaitsev's vs Hoffman's rule by taking the E2 reaction mechanism.
A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown: Co2+ (aq) + 2e → Co(s) Eº=-0.29 volt - Cd2+ (aq) +2e →→ Cd(s) E°= -0.42 volt The actual concentrations are: [Co2+ (aq)] = 0.0006 M, [Cd2+] = 0.149 M. What is the potential in volt of this galvanic cell? (T-298K) Report your answer with 3 places past the decimal point. Do not put unit in your answer.
== A certain half-reaction has a standard reduction potential E red - 1.32 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be…
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M and [Fe²+] = 0.0170 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+ (aq) — Cr²+(aq) + Fe(s) E = V
An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping a cobalt rod in a solution of CoCl2(aq), and connecting them with a wire and a salt bridge. In the cell that is constructed, the metallic zinc is being oxidized. d. The standard cell potential for this electrochemical cell is 0.482 V and two moles of electrons are exchanged per mole of reaction. What is equilibrium constant, K, for the redox reaction described by this electrochemical cell at 298 K?
The emf of a standard X-Y galvanic cell is -2.763V. If the standard half-cell emf for the oxidation of X at the anode is – 3.04V, what is the standard half-cell emf of Y if Y is the cathode?
Consider the following reactions at 298 K: Co^ 2+ (aq)+2 e^ —>Co(s) K^ + (aq) +e^ - -->K (s) a. Write a balanced equation and calculate the cell potential (E*cell) for a spontaneous reduction oxidation reaction. b. Using the spontaneous balanced reaction from part a, calculate the cell potential (E cell) when [Co^ 2+ ]=0.315 M and [K^ + ]=0.258 M at 298 K
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn^2+(0.20 M)|| H+ (test solution)| H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for is –0.76 V. (Enter your answer to two significant figures.) pH =
What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal place. Cu(s) + 2Ag+ (aq) ⇒ Cu²+ (aq) + 2 Ag (s) Note: Reference the Standard reduction potentials at 25 °C table for additional information. K = 0x10 X S