**Reaction: N _{2} + H_{2} → NH_{3} **

**Balanced Reaction: N _{2} + 3 H_{2} → 2 NH_{3} **

Blue spheres represent N (2 blue spheres together = N_{2}):

• **4 molecules N**_{2}

White ones represent H (2 white spheres together = H_{2}):

• **9** **molecules N**_{2}

Calculate how much NH_{3} can be produced by each reactant:

• **From ****4 molecules N**_{2}

${\mathbf{NH}}_{\mathbf{3}}\mathbf{}\mathbf{molecules}\mathbf{=}\mathbf{4}\mathbf{}\overline{){\mathbf{N}}_{\mathbf{2}\mathbf{}}\mathbf{molecules}}\mathbf{\times}\frac{\mathbf{2}\mathbf{}{\mathbf{NH}}_{\mathbf{3}}\mathbf{}\mathbf{molecules}}{\mathbf{1}\mathbf{}\overline{){\mathbf{N}}_{\mathbf{2}}\mathbf{}\mathbf{molecules}}}$

**NH _{3} molecules = 8 molecules**

• **From ****9** **molecules**** H**_{2}

Nitrogen (N_{2}) and hydrogen (H_{2}) react to form ammonia (NH_{3}). Consider the mixture of N_{2} and H_{2} shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H.

How many N_{2} molecules are left over?

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