Draw an electrolytic cell in which Mn²⁺ is reduced to Mn and Sn is oxidized to Sn²⁺. Label the anode and cathode, indicate the direction of electron flow, and write an equation for the half-reaction occurring at each electrode. What minimum voltage is necessary to drive the reaction?

Verified step by step guidance

1. Step 1: Draw a container divided into two halves. In one half, place a Mn electrode immersed in a Mn2+ solution. In the other half, place a Sn electrode immersed in a Sn2+ solution. Connect the two electrodes with a wire and a battery. This is your basic setup for an electrolytic cell.
2. Step 2: Label the electrode where oxidation occurs as the anode. In this case, Sn is oxidized to Sn2+, so the Sn electrode is the anode. Write the half-reaction for this process: Sn -> Sn2+ + 2e-.
3. Step 3: Label the electrode where reduction occurs as the cathode. In this case, Mn2+ is reduced to Mn, so the Mn electrode is the cathode. Write the half-reaction for this process: Mn2+ + 2e- -> Mn.
4. Step 4: Indicate the direction of electron flow. In an electrolytic cell, electrons flow from the anode to the cathode through the wire. So, draw an arrow on the wire pointing from the Sn electrode to the Mn electrode.
5. Step 5: To find the minimum voltage necessary to drive the reaction, look up the standard reduction potentials for the two half-reactions. The voltage needed is the difference between the two potentials. Remember that in an electrolytic cell, the reaction is non-spontaneous, so the cell potential will be negative. The minimum voltage needed to drive the reaction is the absolute value of the cell potential.

Key Concepts

Electrolytic Cell

An electrolytic cell is a device that uses electrical energy to drive a non-spontaneous chemical reaction. It consists of two electrodes: the anode, where oxidation occurs, and the cathode, where reduction takes place. In this cell, an external power source provides the necessary voltage to facilitate the movement of electrons, allowing the desired chemical transformations to occur.

Half-Reactions

Half-reactions represent the individual oxidation and reduction processes occurring in an electrochemical cell. In this context, the reduction half-reaction involves Mn2+ gaining electrons to form solid Mn, while the oxidation half-reaction involves Sn losing electrons to form Sn2+. Writing these half-reactions helps in understanding the electron transfer and balancing the overall redox reaction.

Minimum Voltage (Electrolysis)

The minimum voltage required to drive an electrolytic reaction is known as the cell potential or decomposition potential. This voltage must overcome the inherent energy barriers of the reactions occurring at the electrodes. It can be calculated using the standard reduction potentials of the half-reactions, and it is essential for ensuring that the desired redox processes occur efficiently in the electrolytic cell.