Question

What mass of sodium nitride is required to produce 14.5g of nitrogen? 2Na3N → N2 + 6Na

Answer 1

Approx....`65*g`..........

Explanation:

You gots the stoichiometric equation.....

`2Na_3N(s) rarr N_2(g) + 6Na(s)`

And this explicitly says that `1*mol` of dinitrogen results from thermolysis of `2*mol` sodium azide....

`"Moles of dinitrogen"=(14.5*g)/(28.01*g*mol^-1)-=0.518*mol`

And thus we need `1.032*mol` of sodium azide, which constitutes a mass of `1.032*molxx65.01*g*mol^-1-=??g`.

Note that there is a highly practical application to this reaction. Apparently it is used to inflate air-bags in autos in the event of an accident.