Just d and e of question please ### Electrochemical Cell ProblemsBelow is a set of questions based on the provided redox reaction for an electrochemical cell. This is an excellent exercise for understanding the concepts of half-reaction, transfer of electrons, cell potential (Eº_cell), equilibrium constant (K), and Gibbs free energy (∆G).**Given Reaction:**\[ \text{Mn(s)} + \text{Sn(NO}_3\text{)}_2\text{(aq)} \rightarrow \text{Sn(s)} + \text{Mn(NO}_3\text{)}_2\text{(aq)} \]#### Questions:1. **Write out the half reaction that occurs at the anode.**2. **How many electrons are transferred?**3. **Calculate the \( E^\circ_{\text{cell}} \) in volts.**4. **Using the \( E^\circ_{\text{cell}} \) value determine the equilibrium constant.**5. **Do you expect the Free Gibbs value to be positive or negative? Use support from parts (c) and (d).** - *(This is a concept question; no calculation should be done!)***Graph/Diagram Explanation:**- There are no graphs or diagrams included in this problem set. This material is designed to help students reinforce their understanding of the basic concepts of electrochemistry. Each part of the question addresses a fundamental aspect necessary for a comprehensive understanding of the subject matter.

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10. Use the following equation answer the questions below. Mn(s) + Sn(NO3)2(aq) → Sn(s) + Mn(NO3)2(aq) a. Write out the half reaction that occurs at the anode. b. How many electrons are transferred? C. Calculate the Ecell in volts. d. Using the Ecell value determine the equilibrium constant. e. Do you expect the Free Gibb's value to be positive or negative? Use support from parts c and d. (This is a concept question; no calculation should be done!)

10. Use the following equation answer the questions below. Mn(s) + Sn(NO3)2(aq) → Sn(s) + Mn(NO3)2(aq) a. Write out the half reaction that occurs at the anode. b. How many electrons are transferred? C. Calculate the Ecell in volts. d. Using the Ecell value determine the equilibrium constant. e. Do you expect the Free Gibb's value to be positive or negative? Use support from parts c and d. (This is a concept question; no calculation should be done!)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 5QRT: Identify each statement as true or false. Rewrite each false statement to make it true. (a)...

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Give the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?
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The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).
A standard galvanic cell is constructed so that the overall cell reaction is 2A13++(aq)+3M(s)3M2+(aq)+2A1(s) Where M is an unknown metal. If G = 411 kJ for the overall cell reaction, identify the metal used to construct the standard cell.
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