Question
How does the removal of CO2 affect the equilibrium system of CO(g) + H2O(g) <=> CO2(g) + H2(g) + 41.2 kJ?
Answers
Answered by
GPT-4o mini
In the given reaction:
\[ \text{CO}(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}_2(g) + \text{H}_2(g) + 41.2 \, \text{kJ} \]
this reaction is an equilibrium system involving the reactants carbon monoxide (CO) and water vapor (H₂O) producing carbon dioxide (CO₂) and hydrogen gas (H₂) while releasing energy (indicated by the positive \( 41.2 \, \text{kJ} \) value).
To understand how the removal of CO₂ affects this equilibrium, we can apply Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change and establish a new equilibrium.
**Effect of removing CO₂:**
- When CO₂ is removed from the system, the concentration of one of the products (CO₂) decreases.
- According to Le Chatelier's principle, the equilibrium will shift to the right (toward the products) to increase the concentration of CO₂ back to restore equilibrium.
- As a result, more CO and H₂O will react to form additional CO₂ and H₂.
Thus, the removal of CO₂ will shift the equilibrium toward the products (right side of the reaction), leading to an increase in the concentrations of CO and H₂O as they are converted to CO₂ and H₂.
\[ \text{CO}(g) + \text{H}_2\text{O}(g) \rightleftharpoons \text{CO}_2(g) + \text{H}_2(g) + 41.2 \, \text{kJ} \]
this reaction is an equilibrium system involving the reactants carbon monoxide (CO) and water vapor (H₂O) producing carbon dioxide (CO₂) and hydrogen gas (H₂) while releasing energy (indicated by the positive \( 41.2 \, \text{kJ} \) value).
To understand how the removal of CO₂ affects this equilibrium, we can apply Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change and establish a new equilibrium.
**Effect of removing CO₂:**
- When CO₂ is removed from the system, the concentration of one of the products (CO₂) decreases.
- According to Le Chatelier's principle, the equilibrium will shift to the right (toward the products) to increase the concentration of CO₂ back to restore equilibrium.
- As a result, more CO and H₂O will react to form additional CO₂ and H₂.
Thus, the removal of CO₂ will shift the equilibrium toward the products (right side of the reaction), leading to an increase in the concentrations of CO and H₂O as they are converted to CO₂ and H₂.