Question

How do we represent the oxidation of a `31.7*g` mass of iron by chlorine gas? What mass of `FeCl_3(s)` results?

Answer 1

`Fe(s) + 3/2Cl_2(g) rarr FeCl_3(s)`

Explanation:

Moles of iron: `(31.7*g)/(55.85* g* mol^-1)` `=` `??*mol`

This molar quantity of iron requires `3/2` molar equivalents of chlorine gas for complete reaction. What is oxidized, and what is reduced in the reaction? How do you know?