Chemistry: Molecular Approach (4th Edition)

Published by Pearson
ISBN 10: 0134112830
ISBN 13: 978-0-13411-283-1

Chapter 2 - Exercises - Page 81: 98


\[\underline{\text{16}\text{.00 g}}\]

Work Step by Step

Calculate the mass of nitrogen as follows: \[\begin{align} & \text{Ratio}=\frac{\text{Mass of nitrogen}}{\text{Mass of}{{\text{ }}^{\text{12}}}\text{C}} \\ & \frac{7}{6}=\frac{\text{Mass of nitrogen}}{\text{12}\text{.00 g/mol }} \end{align}\] Rearrange the above expression as follows: \[\begin{align} & \text{Mass of nitrogen}=\frac{7\times 12.00\text{ g/mol}}{6} \\ & =14.00\text{ g/mol} \end{align}\] Calculate the mass of oxygen in \[{{\text{N}}_{\text{2}}}\text{O}\] as follows: \[\begin{align} & \text{Ratio}=\frac{\text{2}\left( \text{Mass of nitrogen} \right)}{\text{Mass of oxygen}} \\ & \frac{7}{4}=\frac{2\left( 14.00\text{ g/mol} \right)}{\text{Mass of oxygen}} \end{align}\] Rearrange the above expression as follows: \[\begin{align} & \text{Mass of oxygen}=\frac{4\times 2\left( 14.00\text{ g/mol} \right)}{7} \\ & =16.00\text{ g/mol} \end{align}\] The mass of \[1\text{ mol}\] of oxygen atoms is \[\underline{\text{16}\text{.00 g}}\].
Update this answer!

You can help us out by revising, improving and updating this answer.

Update this answer

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.