The following reaction is a redox reaction: CuSO4 (aq) + Ni(s) --> NiSO4 (aq) + Cu(s) a) Write the total ionic equation: __________________________________________________________________ b) Write the net ionic equation: ___________________________________________________________________ c) Write the oxidation and reduction half-cell reactions: Oxidation: _____________________________________________ Eo = ______________ Reduction: ____________________________________________ Eo = ______________ d) Calculate the standard cell potential and determine if the reaction is spontaneous or non-spontaneous.
The following reaction is a redox reaction: CuSO4 (aq) + Ni(s) --> NiSO4 (aq) + Cu(s) a) Write the total ionic equation: __________________________________________________________________ b) Write the net ionic equation: ___________________________________________________________________ c) Write the oxidation and reduction half-cell reactions: Oxidation: _____________________________________________ Eo = ______________ Reduction: ____________________________________________ Eo = ______________ d) Calculate the standard cell potential and determine if the reaction is spontaneous or non-spontaneous.
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter18: Oxidation–reduction Reactions And Electrochemistry
Section: Chapter Questions
Problem 74AP: . To obtain useful electrical energy from an oxidation-reduction process, we must set up the...
Related questions
Question
The following reaction is a
a) Write the total ionic equation: __________________________________________________________________
b) Write the net ionic equation: ___________________________________________________________________
c) Write the oxidation and reduction half-cell reactions:
Oxidation: _____________________________________________ Eo = ______________
Reduction: ____________________________________________ Eo = ______________
d) Calculate the standard cell potential and determine if the reaction is spontaneous or non-spontaneous.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry for Today: General, Organic, and Bioche…
Chemistry
ISBN:
9781305960060
Author:
Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:
Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry for Today: General, Organic, and Bioche…
Chemistry
ISBN:
9781305960060
Author:
Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax