Write the anode reaction and cathode reaction for the Zn-Cu voltaic cell that was prepared in Part 2. Clearly indicate which reaction occurs at the anode and which occurs at the cathode. Use proper notation and formatting

Suppose the galvanic cell sketched below is powered by the following reaction: Mg(s)+CuCl,(aq) MgCl,(aq)+Cu(s) e- E1 E2 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cellI. O- Write a balanced equation for the half-reaction that happens at the anode of this cell. 0,0. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?

*Please write the half-reactions for the anode and cathode and explain if you can. Thank you in advance* Consider the electrolysis of aqueous solutions below. For each, show the species produced at the anode and the cathode. Aqueous FeCl3.

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2 IO3(aq)+12 H*(aq)+10e¯ 1₂(s) + 6H₂O(1) 2+ Cu²+ (aq)+e Cu (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell Yes 1 standard reduction potential = +1.195 V Ered red = +0.153 V