Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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I need help with this question and I know it has three parts but it counts as one question.
Transcribed Image Text:For the following questions, state whether there would be a shift to the right, left, more of a shift to the right or left, or nothing. If asked why a reaction shifts in a particular reason, the answer should be kept simple because it decreases, increases, or does nothing to a specific reactant, product, or nothing to the main reaction. State what the exact reactant is.
For instance, in the reaction below, if something is added that decreases \( \text{NH}_3 \), then write “the reaction shifts to the left because it decreases \( \text{NH}_3 \)”.
![### Equilibrium Reaction Analysis
**3.) For the following equilibrium reaction**
\[ 2NO_2(g) \leftrightarrow N_2O_4(g) + \Delta \]
Refer to the Tro textbook to understand what Le Chatelier's principle states regarding gases. Assume that the reaction is conducted in an enclosed movable piston.
*[Hint: Remember that \( PV = nRT \)]*
**Analysis:**
**a.) The pressure of the reaction is increased.**
- Discuss how increasing pressure affects the equilibrium position according to Le Chatelier’s principle. Consider how the reaction might shift towards the side with fewer moles of gas.
**b.) The volume of the reaction is decreased.**
- Analyze how a decrease in volume, which increases pressure, will impact the equilibrium according to Le Chatelier's principle.
**c.) The volume of the reaction is increased.**
- Evaluate the effects of volume increase, equivalent to pressure decrease, on the reaction's equilibrium position. Discuss how this might favor the reaction producing more moles of gas.](https://content.bartleby.com/qna-images/question/dad50ce8-459c-4858-95e9-e24f7f9ebbc0/add9a2ea-e944-44f7-bd18-e55cfb650239/iheofba_processed.jpeg)
Transcribed Image Text:### Equilibrium Reaction Analysis
**3.) For the following equilibrium reaction**
\[ 2NO_2(g) \leftrightarrow N_2O_4(g) + \Delta \]
Refer to the Tro textbook to understand what Le Chatelier's principle states regarding gases. Assume that the reaction is conducted in an enclosed movable piston.
*[Hint: Remember that \( PV = nRT \)]*
**Analysis:**
**a.) The pressure of the reaction is increased.**
- Discuss how increasing pressure affects the equilibrium position according to Le Chatelier’s principle. Consider how the reaction might shift towards the side with fewer moles of gas.
**b.) The volume of the reaction is decreased.**
- Analyze how a decrease in volume, which increases pressure, will impact the equilibrium according to Le Chatelier's principle.
**c.) The volume of the reaction is increased.**
- Evaluate the effects of volume increase, equivalent to pressure decrease, on the reaction's equilibrium position. Discuss how this might favor the reaction producing more moles of gas.
Expert Solution
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Step 1
LeChatelier's Principle or The Equilibrium law is used to predict the effect of any change in conditions on the chemical equilibrium.
- Change in concentration of any chemical species would the equilibria to that side so that the change can be countered and equilibrium conditions are restored.
- Change in temperature is considered in accordance whether the given reaction is exothermic or endothermic. For and endothermic reaction, increase in temperature shifts the equilibria to right whereas for an exothermic reaction the same change shifts the equilibria to the left.
- Change is pressure affects the equilibria taking into account the difference in number of moles of gas. It is generally studied based on change in volume. An increase in pressure shifts equilibria towards fewer moles whereas decrease in pressure shifts chemical equilibria towards side with more moles.
- Change in volume: An increase in volume shifts the equilibria towards the side with more moles and a decrease in volume favors shifting of equilibria towards side with fewer moles.
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