Consider the galvanic cell based on the following half-reactions: Zn2+ + 2e + Zn e = -0.76 V Cd?+ + 2e → Cd e = -0.40 V %3D a. Determine the overall cell reaction and calculate Ecell (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) E cell b. Calculate AG' and K for the cell reaction at 25°C. AG kJ K = c. Calculate Ecell at 25°C when Zn2+] Ca2+ = 0.10 M and = 7.2 x 10-5 M. Ecell

Consider the galvanic cell based on the following half-reactions: Zn2+ + 2e + Zn e = -0.76 V Cd?+ + 2e → Cd e = -0.40 V %3D a. Determine the overall cell reaction and calculate Ecell (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) E cell b. Calculate AG' and K for the cell reaction at 25°C. AG kJ K = c. Calculate Ecell at 25°C when Zn2+] Ca2+ = 0.10 M and = 7.2 x 10-5 M. Ecell

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

See similar textbooks

Similar questions

For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and 0.750 M? What is the spontaneous reaction?
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.