Apply Le Chatelier's principle and decide how (by altering temperature, pressure, etc.) you could increase the amount of the products in the following reactions: 1) 2CO2 (g) ----> 2CO (g) + O2 (g) AHº=566 kJ 2) 2SO2 (g) + O2 (g) ----> 2SO3 (g)

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# DQ5: Chemical Equilibrium

**Available until Sunday, June 28, 2020 12:59 PM CDT**  
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This discussion fulfills the objective #6 of chapter 15.

Apply Le Chatelier's principle and decide how (by altering temperature, pressure, etc.) you could increase the amount of the products in the following reactions:

1. \(2CO_2(g) \leftrightharpoons 2CO(g) + O_2(g) \quad \Delta H^{0} = 566 \, \text{kJ} \)
2. \(2SO_2(g) + O_2(g) \leftrightharpoons 2SO_3(g) \)

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### Explanation:

**Le Chatelier's Principle:** 

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

### Reaction 1:
\[ 2CO_2(g) \leftrightharpoons 2CO(g) + O_2(g) \quad \Delta H^{0} = 566 \, \text{kJ} \]

For this reaction:
- **Increase Temperature:** Since the reaction is endothermic (\(\Delta H > 0\)), increasing the temperature will push the equilibrium towards the products (right).
- **Changing Pressure:** The number of moles of gases increases from 2 to 3 from reactants to products. Decreasing pressure will favor the formation of more moles of gas (move to the right).

### Reaction 2:
\[ 2SO_2(g) + O_2(g) \leftrightharpoons 2SO_3(g) \]

For this reaction:
- **Increase Pressure:** Since there are fewer moles of gas on the product side (3 to 2), increasing pressure will push the equilibrium towards the products (right).
- **Temperature:** The effect of temperature is not given due to lack of \(\Delta H\) information.

Ensure you start a thread before reading and replying to other threads.
Transcribed Image Text:# DQ5: Chemical Equilibrium **Available until Sunday, June 28, 2020 12:59 PM CDT** **Must post first.** This discussion fulfills the objective #6 of chapter 15. Apply Le Chatelier's principle and decide how (by altering temperature, pressure, etc.) you could increase the amount of the products in the following reactions: 1. \(2CO_2(g) \leftrightharpoons 2CO(g) + O_2(g) \quad \Delta H^{0} = 566 \, \text{kJ} \) 2. \(2SO_2(g) + O_2(g) \leftrightharpoons 2SO_3(g) \) **[Start a New Thread]** _Filter by:_ All Threads _Sort by:_ Oldest Thread _You must start a thread before you can read and reply to other threads_ --- ### Explanation: **Le Chatelier's Principle:** Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. ### Reaction 1: \[ 2CO_2(g) \leftrightharpoons 2CO(g) + O_2(g) \quad \Delta H^{0} = 566 \, \text{kJ} \] For this reaction: - **Increase Temperature:** Since the reaction is endothermic (\(\Delta H > 0\)), increasing the temperature will push the equilibrium towards the products (right). - **Changing Pressure:** The number of moles of gases increases from 2 to 3 from reactants to products. Decreasing pressure will favor the formation of more moles of gas (move to the right). ### Reaction 2: \[ 2SO_2(g) + O_2(g) \leftrightharpoons 2SO_3(g) \] For this reaction: - **Increase Pressure:** Since there are fewer moles of gas on the product side (3 to 2), increasing pressure will push the equilibrium towards the products (right). - **Temperature:** The effect of temperature is not given due to lack of \(\Delta H\) information. Ensure you start a thread before reading and replying to other threads.
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