# How do you write the equation for this reaction: Nitrogen gas and fluorine gas combine to produce nitrogen trifluoride gas?

Jul 5, 2018

$\frac{1}{2} {N}_{2} \left(g\right) + \frac{3}{2} {F}_{2} \left(g\right) \rightarrow N {F}_{3} \left(g\right)$

#### Explanation:

$N {F}_{3}$ is in fact not so nasty .... it is much safer than $N C {l}_{3}$ or $N {I}_{3}$.. Of course the direct synthesis with fluorine gas is the province of specialist inorganic chemists...

Jul 5, 2018

${N}_{2} + 3 {F}_{2} \to 2 N {F}_{3}$

#### Explanation:

Nitrogen molecule is ${N}_{2}$

Flourine molecule is ${F}_{2}$

Nitrogen triflouride is $N {F}_{3}$
(tri- means 3, and $N$ usually has 3 covalent bonds, $F$ has 1,
so 3$F$ to 1$N$)

write unbalanced eqn for reaction

${N}_{2} + {F}_{2} \to N {F}_{3}$ (not balanced)

now balance the number of atoms on each side:
at least 2 atoms of nitrogen so at least 2 molecules of $N {F}_{3}$
2 molecules of $N {F}_{3}$ need 6 $F$ atoms = 3 ${F}_{2}$ molecules.

${N}_{2} + 3 {F}_{2} \to 2 N {F}_{3}$ (now balanced, 2$N$ and 6$F$ atoms each side)