Question
Nitrogen monoxide (NO) is $46.7 \%$ nitrogen by mass. Use the law of multiple proportions to calculate the mass percentage of nitrogen in nitrogen dioxide ( $\mathrm{NO}_{2}$ ).
Step 1
7 \%$ nitrogen by mass. This means that the remaining mass is due to oxygen, which is $100\% - 46.7\% = 53.3\%$. Show more…
Show all steps
Your feedback will help us improve your experience
Amy Jiang and 101 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
$\mathrm{NO}_{2}$ (nitrogen dioxide) and $\mathrm{N}_{2} \mathrm{O}_{4}$ (dinitrogen tetroxide) have the same empirical formula, NO$_{2}$ . Confirm this by calculating the percent by mass of each element present in the two compounds.
Chemical Composition
Calculation of Molecular Formulas
Use the atomic masses given on the inside front cover of the text to calculate the mass percentages of nitrogen and oxygen in dinitrogen oxide.
Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide. $$2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{~g})$$ Starting with $2.2 \mathrm{~mol} \mathrm{NO},$ calculate how many moles and how many grams of $\mathrm{O}_{2}$ are required for complete reaction. Calculate what mass of $\mathrm{NO}_{2}$, in grams, is produced.
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD