Question

How many grams of salt are required to produce a `355*mg` mass of chlorine gas?

Answer 1

Of chlorine gas, `Cl_2`..........?

Explanation:

`NaCl(s) rarr Na(s) + 1/2Cl_2(g)`.

We require `(0.355*g)/(70.90*g*mol^-1)=0.00500*mol`.

Given the stoichiometry, we require at least `0.0100*mol` salt, i.e. `0.0100*molxx58.44*g*mol^-1=0.585*g`.

This would not be a terribly efficient way to produce chlorine gas.