Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![Suppose a 250. mL flask is filled with 0.90 mol of H₂ and 0.40 mol of NH₃. This reaction becomes possible:
\[ \text{N}_2 (g) + 3\text{H}_2 (g) \rightleftharpoons 2\text{NH}_3 (g) \]
Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium.
Use \( x \) to stand for the unknown change in the molarity of \(\text{N}_2\). You can leave out the \( M \) symbol for molarity.
| | N₂ | H₂ | NH₃ |
|------------|------------|------------|------------|
| initial | | | |
| change | x | | |
| equilibrium| | | |
The coefficients in the chemical equation indicate the ratio in which the reactants and products will change. This needs to be considered when calculating the changes in molarity and equilibrium values for each compound.](https://content.bartleby.com/qna-images/question/a21199a8-7a5a-4751-9685-1126762a8cde/bc380c9e-7116-4187-bc56-20bef2f0e1e5/3ywynqp_processed.png)
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.90 mol of H₂ and 0.40 mol of NH₃. This reaction becomes possible:
\[ \text{N}_2 (g) + 3\text{H}_2 (g) \rightleftharpoons 2\text{NH}_3 (g) \]
Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium.
Use \( x \) to stand for the unknown change in the molarity of \(\text{N}_2\). You can leave out the \( M \) symbol for molarity.
| | N₂ | H₂ | NH₃ |
|------------|------------|------------|------------|
| initial | | | |
| change | x | | |
| equilibrium| | | |
The coefficients in the chemical equation indicate the ratio in which the reactants and products will change. This needs to be considered when calculating the changes in molarity and equilibrium values for each compound.
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