You have two beakers. One beaker contains 1 M Hg²* and 1 M Hg22*. The second beaker contains 1 M Fe2* and 1 M Fe*. All metals are present as their soluble nitrate salts. Design and draw a galvanic cell using these solutions (if you need other materials to complete the cell, you may add them in – state what they are needed for). Show the direction the electrons move (and where they move) and label the cathode and anode. Give the net ionic equation for the spontaneous reaction taking place in this galvanic cell. What would E°sell be?

42) A positive number for maximum useful work in a spontaneous process (voltaic cell) indicates that the cell will perform work on its surroundings. 41) The standard reduction potential of X is 1.23 V and that of Y is -0.44 V therefore X is oxidized by Y. 40) In a half reaction the amount of a substance that is reduced or oxidized is directly proportional to the number of electrons generated in the cell. 39) The standard reduction potential, Ered is proportional to the stoichiometric coefficient.

Describe what is happening at the anode and cathode in a voltaic cell between copper (submerged in copper (II) sulfate) and iron (submerged in iron (II) sulfate). Reference Appendix L in the OpenStax textbook.

For each of the reactions, label the half-reaction that is the anode and the reaction that is the cathode in a Galvanic CellI. 1. Cu(s) + 2 Ag*(aq) → Cu²+(aq) + 2 Ag(s) → Zn2+(aq) + H2(g) 2. Zn(s) + 2H*(aq) → Cu(s) → Cu2+(aq) + 2e Choose... + Ag*(aq) + 1e → Ag(s) Choose... + Zn(s) Zn(s) → Zn2+(aq) + 2e Choose... + 2H*(aq) + 2e → H2(g) Choose... + Don Choose... anode cathode

Explain the process of electrolysis using the diagram below. Where does oxidation occur? Where does reduction occur? Describe the direction of the flow of electrons. How is this electrolytic cell different from a voltaic cell? Note: The symbol Me stands for a metal.   Show all work and answer in complete sentences.

Which of the following is a true statement regarding an electrolytic cell?     Oxidation occurs at the cathode.     Electrons flow from the cathode to the anode.     All these statements are true.     Electrical energy is used to cause a chemical reaction to occur that would be otherwise be nonspontaneous.

Consider a galvanic cell based on the following half reactions: E (V) M4+ + 4e M 0.66 N3+ ++3e N 0.10 Assuming the value of Faraday's constant is 96,485 C/mol e, the value of AG° for this cell is J

All of the following statements regarding electrochemical cells are true except All electrochemical cells require an applied electric current. In a voltaic cell the electrons flow from the anode to the cathode. In a voltaic cell, the half reactions are separated. The salt bridge maintains electricalcontact and charge neutrality.

A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H (aq) +Se Fe³+ (aq) +e 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. half-reaction Write a balanced. equation for the Answer the following questions about this cell. 0 - Mn² (aq) + 4H₂O(1) Fe (aq) standard reduction potential +1.51 V Ered=+0.771 V 20 "red =

2.Write a balanced cell reaction. Include the phases of all species in the chemical equation.