Combine the two half-reactions that give the spontaneous cell reaction with the smallest e∘. fe2+(aq)+2e−→fe(s) e∘=−0.45v i2(s)+2e−→2i−(aq) e∘=0.54v cu2+(aq)+2e−→cu(s) e∘=0.34v

The spontaneous cell reaction having smallest is

Explanation:

We are given:

The substance having highest positive potential will always get reduced and will undergo reduction reaction. Here, iodine will always undergo reduction reaction, then copper and then iron.

The equation used to calculate electrode potential of the cell is:

The combination of the cell reactions follows:

Here, iodine is getting reduced and iron is getting oxidized.

The cell equation follows:

Oxidation half reaction:    

Reduction half reaction:    

Thus, this cell will not give the spontaneous cell reaction with smallest

Here, iodine is getting reduced and copper is getting oxidized.

The cell equation follows:

Oxidation half reaction:    

Reduction half reaction:  

Thus, this cell will give the spontaneous cell reaction with smallest

Here, copper is getting reduced and iron is getting oxidized.

The cell equation follows:

Oxidation half reaction:    

Reduction half reaction:    

Thus, this cell will not give the spontaneous cell reaction with smallest

Hence, the spontaneous cell reaction having smallest is

the answer is the

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of c is as shown here in the image.