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!)