A student measures the potential of a cell made up with 1 MNISO, in one solution and 1 MAGNO, in the other. There is a nickel electrode in the NISO, and a silver electrode in the AgNO,. The student finds the potential of the cell, E to be 1.07 V, and that the nickel electrode is negative. Show complete calculations for the following questions. 1. At which electrode is oxidation occurring?
A student measures the potential of a cell made up with 1 MNISO, in one solution and 1 MAGNO, in the other. There is a nickel electrode in the NISO, and a silver electrode in the AgNO,. The student finds the potential of the cell, E to be 1.07 V, and that the nickel electrode is negative. Show complete calculations for the following questions. 1. At which electrode is oxidation occurring?
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...
Related questions
Question
Equation 8 refered to in question 7 is Ecell = Eocell - 0.0592/n • log([D2+]d/[B+]b)
Transcribed Image Text:A student measures the potential of a cell made up with 1 M NiSO₄ in one solution and 1 M AgNO₃ in the other. There is a nickel electrode in the NiSO₄ and a silver electrode in the AgNO₃. The student finds the potential of the cell E° to be 1.07 V and that the nickel electrode is negative. Show complete calculations for the following questions.
1. At which electrode is oxidation occurring?
2. Write the half-reaction taking place at the anode:
3. Write the half-reaction taking place at the cathode:
4. What is E°₀(cell) given that the potential of the silver, silver ion electrode, E°₀ Ag⁺/Ag, is taken to be 0.00 V?
________ V
![**Voltaic Cells**
5. If \( E^\circ_{\text{cell}} \) equals 0.80 V, what is \( E^\circ_{\text{anode}} \)?
\_\_\_\_\_\_\_\_ V
6. Write the net ionic equation for the reaction that occurs in the cell studied by the student:
\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_
7. The student adds 6 M NH\(_3\) to the NFSO\(_{3(s)}\) solution that has \( \text{NiNH}_3^{2+} \) as the nickel ion. The cell voltage \( E_{\text{cell}} \) decreases to 1.43 V, and the nickel electrode is still negative. Find the concentration of \( N^{2+} \) ion in the cell (use Equation (8)). Show your calculations.
\_\_\_\_\_\_\_\_\_
8. In question 7, the \([ \text{NiNH}_3^{2+} ] \) is about 0.01 M, and \([ \text{NH}_3 ]\) is about 3 M. Given these values and \([ \text{Ni}^{2+} ]\) from question 7, determine \( K \) for the following reaction. Show your calculations.
\( \text{NiNH}_3^{2+} \, ( \text{aq} ) \rightarrow \text{Ni}^{2+} \, ( \text{aq} ) + 6 \, \text{NH}_3 \, ( \text{aq} ) \)
\( K = \_\_\_\_\_\_\_\_\_\_\_ \)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4577927b-541a-4496-92af-4aa8842e3cf6%2F2e813cc4-5b3f-43d4-bc01-ff5a1fd007b5%2F5uzxnnn.jpeg&w=3840&q=75)
Transcribed Image Text:**Voltaic Cells**
5. If \( E^\circ_{\text{cell}} \) equals 0.80 V, what is \( E^\circ_{\text{anode}} \)?
\_\_\_\_\_\_\_\_ V
6. Write the net ionic equation for the reaction that occurs in the cell studied by the student:
\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_
7. The student adds 6 M NH\(_3\) to the NFSO\(_{3(s)}\) solution that has \( \text{NiNH}_3^{2+} \) as the nickel ion. The cell voltage \( E_{\text{cell}} \) decreases to 1.43 V, and the nickel electrode is still negative. Find the concentration of \( N^{2+} \) ion in the cell (use Equation (8)). Show your calculations.
\_\_\_\_\_\_\_\_\_
8. In question 7, the \([ \text{NiNH}_3^{2+} ] \) is about 0.01 M, and \([ \text{NH}_3 ]\) is about 3 M. Given these values and \([ \text{Ni}^{2+} ]\) from question 7, determine \( K \) for the following reaction. Show your calculations.
\( \text{NiNH}_3^{2+} \, ( \text{aq} ) \rightarrow \text{Ni}^{2+} \, ( \text{aq} ) + 6 \, \text{NH}_3 \, ( \text{aq} ) \)
\( K = \_\_\_\_\_\_\_\_\_\_\_ \)
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 2 steps
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
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY