Question

Calculate the cell potential for the reaction as written at 25.00 °C , given that [Mg2+]=0.808 M and [Sn2+]=0.0120 M . Use the standard reduction potentials in this table. Mg(s)+Sn2+(aq) ⇌ Mg2+(aq)+Sn(s)

Answer 1

To calculate the cell potential for the given reaction, you can use the Nernst equation.

Step-by-step explanation:

To calculate the cell potential for the given reaction, you can use the Nernst equation. The Nernst equation relates the cell potential to the concentrations of the reactants and products in the half-cells. The equation is:

Ecell = E°cell - (0.0592 / n) * log(Q)

where E°cell is the standard cell potential, n is the number of electrons transferred, and Q is the reaction quotient. In this case, the reaction is:

Sn2+ (aq) + Mg(s) → Sn(s) + Mg2+ (aq)

The standard cell potential can be determined using the reduction potentials from the given table:

Sn2+ (aq) + 2e- → Sn(s) E° = -0.14 V

Mg2+ (aq) + 2e- → Mg(s) E° = -2.37 V

By substituting the values into the Nernst equation, you can calculate the cell potential.

Answer 2

To calculate the cell potential for the given reaction, we use the Nernst equation. The cell potential is -2.2451 V.

Step-by-step explanation:

To calculate the cell potential for the given reaction, we need to find the reduction potentials for each half-cell and apply the Nernst equation.

The reduction potential for the Mg2+/Mg half-reaction is -2.37 V and for the Sn2+/Sn half-reaction is -0.136 V. To calculate the cell potential, we use the equation:

Ecell = E°cell - (0.0592 V/n) × log([Mg2+]/[Sn2+]),

where E°cell is the standard cell potential, n is the stoichiometric coefficient of the electrons, and [Mg2+] and [Sn2+] are the concentrations of the ions.

Plugging in the values, we get:

Ecell = (-2.37 V) - (0.0592 V/2) × log(0.808/0.0120) = -2.37 V + 0.0296 V × log(67.3) = -2.37 V + 0.0296 V × 4.212 = -2.37 V + 0.1249 V = -2.2451 V.

Therefore, the cell potential for the reaction as written at 25.00 °C is -2.2451 V.