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

Question

2362 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-02-15T06:18:19

Of chlorine gas, $Cl_2$ ..........?

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

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.

How many grams of salt are required to produce a 355*mg355*mg mass of chlorine gas?