🤓 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.

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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 Mass Percent Formula concept. You can view video lessons to learn Mass Percent Formula. Or if you need more Mass Percent Formula practice, you can also practice Mass Percent Formula practice problems.

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