Questions and Answers
Which compound will cause a shift in equilibrium due to a common ion effect?
What will happen to the chemical equilibrium if NH4Cl is added to this solution?
The chemical equilibrium will shift to the left.
What will happen to the chemical equilibrium if HCl is added to the system?
The chemical equilibrium will shift to the left.
What will happen if the pressure of the system is increased for the reaction 2H2(g) + O2(g) 2H2O(g)?
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What will happen to the equilibrium of the reaction CH4(g) + H2O(g) CO(g) + 3H2(g) if the pressure is increased?
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What always happens to the equilibrium of a reaction when the temperature is reduced according to Le Chatelier's principle?
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The equilibrium constant changes with a change in temperature.
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What is the definition of a common ion as it applies to Le Chatelier's principle?
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According to Le Chatelier's principle, what is the value of K when equilibrium is established for aA(aq) + bB(aq) cC(aq) + dD(aq)?
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What is the reaction quotient, Q, for the system when [H2] = 0.100 M, [I2] = 0.200 M, and [HI] = 3.50 M for the reaction H2(g) + I2(g) 2HI(g)?
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Study Notes
Chemical Equilibrium Principles
- The reaction H2SO4(aq) ⇌ 2H⁺(aq) + SO4²⁻(aq) will shift left if MgSO4 is added due to a common ion effect.
- Addition of NH4Cl to the NH4OH(aq) ⇌ NH4⁺(aq) + OH⁻ reaction shifts equilibrium to the left.
- Adding HCl to H2SO4(aq) ⇌ 2H⁺ + SO4²⁻ shifts equilibrium to the left, increasing H⁺ concentration.
- For the equilibrium reaction 2H2(g) + O2(g) ⇌ 2H2O(g), increasing pressure favors the forward reaction, producing more water.
- In the reaction CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g), increasing pressure shifts equilibrium to the left, favoring the reverse reaction.
Le Chatelier's Principle
- Reducing temperature shifts equilibrium in the exothermic direction, favoring heat release.
- The equilibrium constant (K) varies with temperature changes but remains constant with changes in concentration or pressure.
- A common ion is defined as an ion that is found in both the equilibrium system and a compound added to the system.
Reaction Quotient and Calculations
- For the equilibrium reaction aA(aq) + bB(aq) ⇌ cC(aq) + dD(aq), adding reactants or products affects equilibrium but K remains unchanged.
- The reaction quotient (Q) is calculated for H2(g) + I2(g) ⇌ 2HI(g) with [H2] = 0.100 M, [I2] = 0.200 M, and [HI] = 3.50 M, yielding a value of 613.
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Description
Test your understanding of chemical equilibrium and the common ion effect with this quiz. Explore how the addition of different compounds can impact equilibrium in various chemical reactions. Engage with flashcards designed to enhance your knowledge of dynamic equilibria.
