🤓 Based on our data, we think this question is relevant for Professor Ballester's class at NSU.

**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?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ballester's class at NSU.