Textbook Question
When the following equilibria are disturbed by increasing the pressure, does the concentration of reaction products increase, decrease, or remain the same?2 CO2(g) ⇌ 2 CO(g) + O2(g)
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15. Chemical Equilibrium
Le Chatelier's Principle
1:12 minutesProblem 65
Textbook Question
The reaction H2(g) + I2(g) ⇌ 2 HI(g) has ∆H = -2.2 kcal/mol (-9.2 kJ/mol). Will the equilibrium concentration of HI increase or decrease whenH2 is removed?
Verified step by step guidance1
Identify the type of reaction: The given reaction is an exothermic reaction, as indicated by the negative \( \Delta H \) value.
Understand Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
Analyze the effect of removing \( H_2 \): Removing \( H_2 \) will decrease its concentration, causing the equilibrium to shift towards the reactants to produce more \( H_2 \).
Determine the impact on \( HI \) concentration: As the equilibrium shifts towards the reactants, the concentration of \( HI \) will decrease because the reaction will favor the reverse process to produce more \( H_2 \) and \( I_2 \).
Conclude the effect: Therefore, the equilibrium concentration of \( HI \) will decrease when \( H_2 \) is removed.
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Video duration:
1mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Le Chatelier's Principle
Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In this case, removing H2 will shift the equilibrium position to favor the production of H2 to compensate for its loss.
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The following is an endothermic reaction where Kc = 6.73 x 103.For each of the choices below predict in which direction the reaction will proceed
Equilibrium Constant (K)
The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Changes in concentration of reactants or products can affect the position of equilibrium but not the value of K itself.
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Endothermic and Exothermic Reactions
Reactions can be classified as endothermic or exothermic based on the heat absorbed or released. The given reaction is exothermic (∆H = -2.2 kcal/mol), meaning it releases heat. Understanding the nature of the reaction helps predict how changes in concentration will affect the equilibrium position.
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