Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25�c. (the equation is balanced.)

3 cl2(g) + 2 fe(s) --> 6 cl-(aq) + 2 fe3+(aq)

cl2(g) + 2 e- --> 2 cl-(aq); e� = +1.36 v

fe3+(aq) + 3 e- --> fe(s); e� = -0.04 v

+1.32 v

-1.32 v

-1.40 v

+1.40 v

+4.16 v

+ 1.40 V

Explanation:

The balanced chemical equation is:

Here Fe undergoes oxidation by loss of electrons, thus act as anode. Chlorine undergoes reduction by gain of electrons and thus act as cathode.

Where both are standard reduction potentials.

The standard cell potential for the reaction is +1.40 V

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.