What is the standard cell potential for the reaction 2 Cr + 3 Pb²⁺ → 3 Pb + 2 Cr³⁺?Standard Reduction PotentialsE° (V)Pb²⁺(aq) + 2e⁻ → Pb(s)-0.13Cr³⁺(aq) + 3e⁻ → Cr(s) -0.74

To calculate the standard cell potential for the reaction, we need to use the standard reduction potentials given.

The reaction is: 2 Cr + 3 Pb²⁺ → 3 Pb + 2 Cr³⁺

First, we need to identify the oxidation and reduction reactions.

Cr is being oxidized to Cr³⁺ (losing electrons), and Pb²⁺ is being reduced to Pb (gaining electrons).

The standard reduction potential for the reduction of Pb²⁺ to Pb is -0.13 V.

However, since the reaction is actually the oxidation of Cr to Cr³⁺, we need to reverse the sign of the standard reduction potential for Cr³⁺ to Cr, which is -0.74 V, making it +0.74 V.

The standard cell potential (E°cell) is the sum of the standard reduction potential for the reduction half-reaction and the standard reduction potential for the oxidation half-reaction.

So, E°cell = E°red (reduction) + E°red (oxidation)

Substituting the values in, we get:

E°cell = -0.13 V + 0.74 V = 0.61 V

So, the standard cell potential for the reaction is 0.61 V.