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

We’re asked to **calculate the percent nitrogen by mass** in **glycine** based on its **molecular model****.**

Recall the **mass percent formula**:

$\overline{){\mathbf{\%}}{\mathbf{}}{\mathbf{mass}}{\mathbf{=}}\frac{\mathbf{mass}\mathbf{}\mathbf{component}}{\mathbf{total}\mathbf{}\mathbf{mass}}{\mathbf{\times}}{\mathbf{100}}}$

The ** %N by mass in glycine** can be calculated using the equation:

$\overline{){\mathbf{\%}}{\mathbf{}}{\mathbf{mass}}{\mathbf{}}{\mathbf{N}}{\mathbf{=}}\frac{\mathbf{mass}\mathbf{}\mathbf{N}\mathbf{}\mathbf{in}\mathbf{}\mathbf{glycine}}{\mathbf{molar}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{glycine}}{\mathbf{\times}}{\mathbf{100}}}$

To do so, we need to **determine the molecular formula of glycine** and its **molar mass**.

First, we need to **identify the element represented by each sphere** based on its **color**.

Recall the** color schemes** used for a molecular model:

__white__= Hydrogen, H**red**= Oxygen, O**blue**= Nitrogen, N**black**= Carbon, C

Glycine, an amino acid used by organisms to make proteins, is represented by the molecular model below.

Calculate the percent nitrogen by mass in glycine.