Calculate the standard cell potential, ∘cell, for the equation Co(s)+F2(g)⟶Co2+(aq)+2F−(aq) Use the table of standard reduction potentials. ∘cell=

3.15 V

Explanation:

Step 1: Write the balanced cell reaction

Co(s) + F₂(g) ⟶ Co²⁺(aq) + 2 F⁻(aq)

Step 2: Identify both half-reactions:

Cathode (reduction): F₂(g) + 2 e⁻ ⟶ 2 F⁻(aq)    E°red = 2.87 V

Anode (oxidation): Co(s) ⟶ Co²⁺(aq) + 2 e⁻      E°red = -0.28 V

Step 2: Calculate the standard cell potential

We will use the following expression.

E°cell = E°red,cathode - E°red,anode

E°cell = 2.87 V - (-0.28 V) = 3.15 V

Given E°cell > 0, the reaction is spontaneous.

if you're asking what comes out, it's steam.

the correct answer is:

a. formation of precipitation