[objectivist]

Hey Everyone. I have been trying to do this problem and keep getting the wrong answer:


A proposed automobile battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a battery to operate 9 h and deliver 1.5 A of current, what is the minimum mass of zinc that the anode must contain?




This is how I tried to do it:
(Maybe its the whole "minimum mass" thing?

9 hours x 120 = 1080 seconds

Charge = current (A)x time (s)
Charge = 1.5 x 1080
Charge = 1620

mol e- = 1620 C (1mole-/96,500 C)
mol e- = 0.0167876

0.0167876 (1 mol Zn?/ 1? mol e- ) ( 65.39g/mol)

I dont know if i did that right...i dont know which molar mass to use, and I dont know how many moles of electrons there are...Please *delete me*
                         

[Borek]

Not checking details, but at first sight: the idea is OK.

However, you are wrong assuming 1 mol Zn/1 mol e- as there are two electrons per every Zn atom.