What statement(s) best describes what occurs when molten NaCL undergoes electrolysis?

Question

I. Cl2(g) is produced at the anode.

II. Na metal is produced at the cathode.

III. The reaction generates a current spontaneously.

a. I & II

b. I & III

c. II & III

d. I, II, & III

e. III only

The answer is A... but why?

Answer 1

I'll assume that anode and cathode mean what I think they still mean. lll cannot be right because electrolysis means an external current is being supplied. The molten salt wont generate its own current.

l and ll indeed are what will occur. The ions will come out of solution as free elements, because the electrons are now supplied by an external source. The chlorine will bubble out at one electrode, and the sodium will be plated out at the other electrode. This is also assuming that the electrodes are made out of a nonreacting material like graphite.

Answer 2

Chlorine is oxidized at the anode, Cl- to Cl, and sodium is reduced at the cathode Na+ to Na.