Consider a Cell Composed of Tin Metal and Zinc Metal

a) Which is the reduction reaction?

The reduction reaction is the reaction that occurs at the zinc electrode, which is Zn²⁺(aq) + 2e⁻ → Zn(s).

b) Which is the oxidation reaction?

The oxidation reaction is the reaction that occurs at the tin electrode, which is Sn(s) → Sn²⁺(aq) + 2e⁻.

c) Write the overall reaction

The overall reaction is: Sn(s) + Zn²⁺(aq) → Sn²⁺(aq) + Zn(s).

d) Calculate the voltage for this cell

The overall voltage for the cell is the difference between these two potentials is -0.62 V.

e) Label the following on the diagram

Zn electrode | Zn(NO₃)₂ || SnSO₄ | Sn electrode

f) What will happen to the mass of each electrode as the reaction proceeds?

As the reaction proceeds, the mass of the tin electrode will decrease as tin atoms are oxidized to form Sn²⁺ ions.

To calculate the voltage for this cell, we need to use the standard reduction potentials for the half reactions. The standard reduction potential for the reduction reaction is -0.76 V, and the standard reduction potential for the oxidation reaction is -0.14 V. The overall voltage for the cell is the difference between these two potentials: Ecell = Ered - Eox = (-0.76 V) - (-0.14 V) = -0.62 V.

In a galvanic cell, the reduction reaction occurs at the cathode, while the oxidation reaction occurs at the anode. In this case, the zinc electrode is the cathode, where Zn²⁺ ions are reduced to form zinc atoms. The tin electrode is the anode, where tin atoms are oxidized to form Sn²⁺ ions.

The overall reaction occurs spontaneously, as the standard reduction potential for the reduction reaction is more positive than the standard reduction potential for the oxidation reaction. This means that the electrons will flow from the anode to the cathode, generating an electrical current.

The salt bridge is used to maintain charge neutrality in the two half-cells, as the electrons flow from the anode to the cathode, and ions must move to balance the charges. Na⁺ ions move towards the anode, while NO³⁻ ions move towards the cathode. This allows for the flow of ions to maintain charge neutrality in both half-cells.

As the reaction proceeds, the mass of the tin electrode will decrease as tin atoms are oxidized to form Sn²⁺ ions. Conversely, the mass of the zinc electrode will increase as zinc ions are reduced to form zinc atoms. This is due to the conservation of mass, as the total mass of the system remains constant.