6. Determine the cell voltage for the following cell Fe) + Cd²+ (2) = Fe²+ (29) + Cd(1) when (a) [Fe] =0.10M and [ Cd²+] = 1.0M, and E= +0.080 V (Done in Lectures) (b) [Fe²+] = 1.0M and [Ca] = 0.010M E= -0.01 V 7. Calculate the equilibrium constant for the reaction in (6) above. NB. At equilibrium, E=0 K=1.05
6. Determine the cell voltage for the following cell Fe) + Cd²+ (2) = Fe²+ (29) + Cd(1) when (a) [Fe] =0.10M and [ Cd²+] = 1.0M, and E= +0.080 V (Done in Lectures) (b) [Fe²+] = 1.0M and [Ca] = 0.010M E= -0.01 V 7. Calculate the equilibrium constant for the reaction in (6) above. NB. At equilibrium, E=0 K=1.05
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Chapter22: An Introduction To Electroanalytical Chemistry
Section: Chapter Questions
Problem 22.17QAP
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![6. Determine the cell voltage for the following cell
Fe) + Cd²+ (2) = Fe²+ (29) + Cd(1)
when (a) [Fe] =0.10M and [ Cd²+] = 1.0M, and E= +0.080 V (Done in Lectures)
(b) [Fe²+] = 1.0M and [Ca] = 0.010M E= -0.01 V
7. Calculate the equilibrium constant for the reaction in (6) above. NB. At equilibrium, E=0
K=1.05](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1153c810-9dd5-41d3-981a-dc931e0e573e%2F55ebba32-6350-4af8-9d73-c875609e55d5%2Fwyj47kc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:6. Determine the cell voltage for the following cell
Fe) + Cd²+ (2) = Fe²+ (29) + Cd(1)
when (a) [Fe] =0.10M and [ Cd²+] = 1.0M, and E= +0.080 V (Done in Lectures)
(b) [Fe²+] = 1.0M and [Ca] = 0.010M E= -0.01 V
7. Calculate the equilibrium constant for the reaction in (6) above. NB. At equilibrium, E=0
K=1.05
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