Chemistry: Atoms First (2nd Edition)

Published by Cengage Learning
ISBN 10: 1305079248
ISBN 13: 978-1-30507-924-3

Chapter 12 - Exercises - Page 524d: 45

Answer

$$K = 3.4$$

Work Step by Step

- The exponent of each concentration is equal to its balance coefficient. $$K = \frac{[Products]}{[Reactants]} = \frac{[ SO_3 ][ NO ]}{[ SO_2 ][ NO_2 ]}$$ 1. Draw the ICE table for this equilibrium: $$\begin{vmatrix} Compound& [ SO_2 ]& [ NO_2 ]& [ SO_3 ]& [ NO ]\\ Initial& 2.00 & 2.00 & 0 & 0 \\ Change& -x& -x& +x& +x\\ Equilibrium& 2.00 -x& 2.00 -x& 0 +x& 0 +x\\ \end{vmatrix}$$ 2. At equilibrium, these are the concentrations of each compound: $ [ SO_2 ] = 2.00 \space M - x$ $ [ NO_2 ] = 2.00 \space M - x$ $ [ SO_3 ] = 0 \space M + x$ $ [ NO ] = 0 \space M + x$ 3. Using the concentration of $ NO $ at equilibrium, find x: $ 0 + x = 1.30 $ $ x = 1.30 - 0 $ $x = 1.30 $ $ [ SO_2 ] = 2.00 \space M - 1.30 =0.700 $ $ [ NO_2 ] = 2.00 \space M - 1.30 =0.700 $ $ [ SO_3 ] = 0 \space M + 1.30 =1.30 $ $ [ NO ] = 0 \space M + 1.30 =1.30 $ - The exponent of each concentration is equal to its balance coefficient. $$K = \frac{[Products]}{[Reactants]} = \frac{[ SO_3 ][ NO ]}{[ SO_2 ][ NO_2 ]}$$ 4. Substitute the values and calculate the constant value: $$K = \frac{( 1.30 )( 1.30 )}{( 0.700 )( 0.700 )} = 3.4$$
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.