Calculate the standard reaction potential and use the half-reaction method to determine the moles of electrons per reaction.  2Au3+(aq) + 3Zn(s) --> 2Au(s) + 3Zn2+(aq)

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential CrO2−4 (aq)+4H2O(l)+3e−→  CrOH3(s)+5OH−(aq) =E0red−0.13V Cl2(g)+2e−→  2Cl−(aq) =E0red+1.359V   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 voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits. V

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe2+(aq) + 2 e– → Fe(s); E° = –0.41 V Pt2+(aq) + 2 e– → Pt(s); E° = 1.18 V Cr2O72–(aq) + 14 H+(aq) + 6 e– → 2 Cr3+(aq) + 7 H2O(); E° = 1.33 V Which of the following is the strongest oxidizing agent? Fe Pt Cr^3+ Fe^2+ Cr2O7^2-

Calculate the standard cell potential and note whether the reaction is spontaneous under standard conditions. Mg(s) + Cu2+ --> Mg2+ + Cu(s)