Question

1.    Upon heating, NaN_3(s) decomposes to Na_(l) and N_2(g). This reaction serves as a convenient laboratory preparation of pure nitrogen gas.

2 NaN_3(s) ¾® 2 Na_(l) + 3 N_2(g)

a)       What number of moles of NaN₃ is required to prepare 1.00 mol of N₂?

 

 

 

b)      What mass of N₂ is produced by the decomposition of 2.00 mol NaN₃? (

 

 

 

c) What mass of Na is produced when 1.75 g of N₂ is prepared? 

Answer 1

We have given the reaction:

$2NaN_3 \rightarrow 2Na+3N_2$

a.) 3 moles of $N_2$ gives 2 moles of $NaN_3$

1 mole of $N_2 \hspace{1mm} gives = \dfrac{2}{3 }$ moles of $NaN_3$

b.) 2 moles of $NaN_3$ gives 1 mole of $N_2$

1 mole of $NaN_3$ give $= \dfrac{1}{3}$ moles of $N_2 = \dfrac{1}{3} \times 28$

c.) Similarly we can also this part also.