Question Bank: Equilibrium

What is a key characteristic of a system at dynamic equilibrium?

In a closed system, if the temperature is increased, how does it affect the equilibrium of an exothermic reaction?

What type of equilibrium can be established in a chemical reaction involving reactants and products?

Which of the following statements is true regarding dynamic equilibrium in a chemical system?

Which process must take place for a dynamic equilibrium to be established?

In the reaction A + B ⇌ C + D, if the concentration of C is increased, what will happen to the equilibrium position?

What defines the extent of a physical process before it reaches equilibrium?

In a dynamic equilibrium, which physical states can be involved?

Which scenario correctly represents chemical equilibrium?

Which factor can disrupt a dynamic equilibrium?

In which type of reaction does dynamic equilibrium commonly occur?

What does it mean if the equilibrium constant (K) for a reaction is very large?

Which principle describes how a system at equilibrium reacts to changes in concentration or pressure?

Which statement best describes a reaction at equilibrium regarding observable properties?

If a chemical equilibrium is disturbed, what is the result according to Le Chatelier's Principle?

What is the condition for a system to be at equilibrium?

In a closed container, if a liquid evaporates, which statement is true at equilibrium?

Which of the following describes dynamic equilibrium?

What happens to the equilibrium when the temperature of a system at equilibrium is increased?

When a sealed container of water is observed, which factor does NOT affect its vapor pressure at equilibrium?

A reaction equilibrium is represented as follows: A + B ⇌ C. If more reactant A is added, what will occur?

What can be inferred if a chemical reaction reaches equilibrium but the concentrations of reactants and products differ significantly?

For the equilibrium expression Kc, what does the 'c' represent?

What effect does adding an inert gas to a system at equilibrium have?

In the context of physical processes, what type of system is necessary to achieve equilibrium?

Calculating Kc for a reaction A + 3B ⇌ 2C, what happens if the concentration of B is reduced?

What does Le Chatelier's principle state regarding equilibrium?

When ions in a saturated solution of a sparingly soluble salt establish equilibrium, what is Ksp?

In a system at equilibrium, if the concentration of a product is increased, according to Le Chatelier's principle, the system will behave how?

What defines a weak electrolyte in an equilibrium context?

What characterizes a dynamic equilibrium in a chemical reaction?

The equilibrium constant K for the reaction A + B ⇌ C + D is defined as which of the following?

If the concentration of a reactant is increased, what will happen to the equilibrium position according to Le Chatelier's principle?

In the reaction 2NO(g) + O2(g) ⇌ 2NO2(g), if NO is removed at equilibrium, what will occur?

Which condition will favor a higher yield of products in the exothermic reaction A + B ⇌ C + D?

What will happen to the equilibrium constant K if the temperature of an exothermic reaction is increased?

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), if 1 mole of N2 and 3 moles of H2 are mixed in a closed container, what is the initial ratio of K?

Which of the following statements is true regarding equilibrium mixtures?

When considering equilibrium constants, what does the term 'activity' refer to?

In an equilibrium reaction, what is the impact of increasing the pressure on a system with unequal moles of gas products and reactants?

If a reaction is at equilibrium, which of the following changes would increase the concentration of the product?

For the equilibrium: 2SO2(g) + O2(g) ⇌ 2SO3(g), which statement correctly describes the equilibrium constant expression?

What does a very large equilibrium constant value indicate about a reaction?

In the context of chemical equilibrium, why is the term 'dynamic' used?

What is the value of the equilibrium constant K if the concentrations at equilibrium are [A]=0.01 M, [B]=0.02 M, [C]=0.03 M, and [D]=0.04 M in the reaction A + B ⇌ C + D?

Which of the following represents a heterogeneous equilibrium?

In a reaction at equilibrium involving a solid, the concentration of the solid is:

For the reaction CaCO3(s) ↔ CaO(s) + CO2(g), what is the expression for the equilibrium constant Kc?

Which factor does not affect the position of a heterogeneous equilibrium?

When the concentration of products increases in a heterogeneous equilibrium, the equilibrium shifts:

At equilibrium for the reaction 2 NOCl(g) ↔ 2 NO(g) + Cl2(g), if Kc = 3.75 × 10^-6, what does this imply about the relative amounts of products to reactants?

For the reaction involving solid and gas, which concentration term is omitted in the Kc expression?

If more of the solid reactant is added to a heterogeneous equilibrium, the system will:

For the equilibrium \( 4 NH_3(g) ightleftharpoons 2 N_2(g) + 6 H_2(g) \), if Δn = 2, what is the relationship between Kp and Kc?

For the equilibrium process \[ CaCO3(s) ightleftharpoons CaO(s) + CO2(g) \], which factor would change the equilibrium position?

For the reaction \( CO2(g) ightleftharpoons C(s) + O2(g) \), what will happen to the equilibrium if the volume of the container is decreased?

If pure water is in equilibrium with water vapor at a certain temperature, the equilibrium involves which physical states?

In the equilibrium reaction \( 2NOCl(g) ightleftharpoons 2NO(g) + Cl2(g) \), what is Δn?

Which of the following is true regarding the equilibrium constant K in a heterogeneous system?

Which of the following defines the equilibrium constant (Kc)?

What happens to the equilibrium position when the concentration of a reactant is increased?

In the equilibrium reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what is the expression for Kc?

Which statement about the equilibrium constant K is true?

What is the value of Kc when the forward reaction is favored, at equilibrium?

If a system at equilibrium is disturbed by removing a product, what will be the result?

Which of the following factors does NOT affect the value of Kc?

What effect does increasing pressure have on equilibrium reactions involving gases?

At equilibrium, 0.5 M of A and 0.1 M of B reflect Kc of 2.5 for the reaction A ⇌ B. What is the concentration of B if [A] is halved?

When heat is added to an exothermic reaction at equilibrium, what direction does the equilibrium shift?

For the reaction H2(g) + I2(g) ⇌ 2HI(g), what effect does reducing the concentration of HI have?

If the system N2(g) + 3H2(g) ⇌ 2NH3(g) at equilibrium changes temperature, how does Kc change?

Which of the following conditions will not affect the value of Kc?

In the reaction 2CO(g) + O2(g) ⇌ 2CO2(g), if 1.0 M of CO2 is added at equilibrium, what will happen?

If the reaction quotient Q is less than the equilibrium constant Kc, which way will the reaction proceed?

For the reaction H2(g) + I2(g) ⇌ 2HI(g), if Kc is 49 at a certain temperature, what can be inferred?

What are the units of Kc for the reaction aA + bB ⇌ cC + dD?

Which principle states that a system at equilibrium will shift to counteract an imposed change?

Which reaction at equilibrium will produce a Kc that is sensitive to temperature changes?

In the equilibrium reaction A + B ⇌ C + D, if D is removed, what will happen?

In the reaction 2NO2(g) ⇌ N2O4(g), if the volume is decreased, what will be the effect on the equilibrium?

If a reaction at equilibrium has a negative ΔG, what does this indicate?

For the reaction 2A(g) ⇌ 2B(g), what happens to Kc when the reaction is doubled?

What happens to Kc at equilibrium if the temperature of an endothermic reaction is increased?

What can you conclude if Kp > Kc at a given temperature for a gaseous reaction?

For a reaction at equilibrium with ΔG=0, which statement is true?

If increasing temperature causes the equilibrium constant Kc to increase, the reaction must be:

In an equilibrium reaction, if the overall reaction produces more moles of gas, what can we infer about the effect of pressure?

What is the primary effect of adding a common ion to a weak acid solution?

According to Le Chatelier's principle, what happens when acetate ions are added to acetic acid?

Which of the following explains the common ion effect?

If the concentration of acetate ion is increased in a solution of acetic acid, what will be observed?

Which factor primarily influences the strength of a weak acid when a common ion is added?

What will happen to the pH of an acetic acid solution when a strong acid is added?

In the dissociation of acetic acid (HAc), what is the role of the acetate ion (Ac-) when added to the solution?

How does adding NaAc to acetic acid affect the ionization constant (Ka)?

Which statement about polyprotic acids is true in the context of the common ion effect?

Why is it harder to remove protons from negatively charged ions in polyprotic acids?

What is the primary chemical equation demonstrating the ionization of acetic acid?

How is the common ion effect observed in a solution containing both acetic acid and sodium acetate?

In a weak acid solution, what happens to the pH when more of the acid is dissolved without a common ion?

If you have a 0.1 M solution of acetic acid and add 0.1 M sodium acetate, what can be inferred about the system?

Which factor must be overcome for a salt to dissolve in a solvent?

What is the typical characteristic of slightly soluble salts?

In which type of solvent would a sparingly soluble salt likely not dissolve?

What primarily influences the solubility of a sparingly soluble salt?

When a salt completely dissolves in a solvent, which of the following is true?

If the solubility product (Ksp) of a salt increases, what does this indicate?

What happens to the solubility of a sparingly soluble salt with increasing temperature typically?

What term describes the energy released when ions are solvated in water?

Which of the following salts is likely to be sparingly soluble in water?

What common misconception exists regarding sparingly soluble salts?

If the temperature of a solution of a sparingly soluble salt is decreased, what is likely to happen?

A salt's dissolution can be described by which of the following equations?

Which ion interaction primarily leads to the solubility of salts in water?

Why do sparingly soluble salts have different solubility levels?

A salt showing high lattice enthalpy is likely to be what in terms of solubility?

Which of the following statements best defines an acid according to Arrhenius's theory?

What occurs when hydrochloric acid is dissolved in water?

Which of the following substances is a strong electrolyte?

Which of the following is a characteristic property of bases?

According to Bronsted-Lowry theory, what is an acid?

What is the pH of a neutral solution at 25 °C?

What is indicated by a pH value of less than 7?

When vinegar is mixed with baking soda, what type of reaction occurs?

What is the primary role of a buffer solution?

How does Le Chatelier's principle predict the response of a system at equilibrium to a change in concentration?

Which of the following statements is true for weak acids?

If the concentration of a weak acid is increased, what happens to the pH of the solution?

What type of ion does a strong base produce in an aqueous solution?

What is the solubility product constant (Ksp) for a sparingly soluble salt?

For the reaction CaCO3(s) ⇌ Ca2+(aq) + CO32-(aq), what happens when more CaCO3 is added to the mixture?

In which type of acid-base reaction is a conjugate base formed?

What distinguishes a Lewis acid from a Bronsted-Lowry acid?

What impact does an inert gas have on the equilibrium of an acid-base reaction in a closed system?

Which of the following best describes a buffer solution?

What components are typically used to prepare an acidic buffer?

Which of the following mixtures would create a buffer solution with a pH around 9.25?

What is the pH relationship used to describe acidic buffer solutions?

A buffer made from acetic acid (pK_a = 4.76) and sodium acetate is found to have a pH of 4.75. If equal amounts of acetic acid and sodium acetate are used, what would be the ratio of their concentrations?

If a buffer solution is diluted, how does its pH change?

Which combination would best describe a buffer solution in biological systems?

Which of the following statements about buffer solutions is false?

What happens to the pH of a buffer when a small amount of strong acid is added?

For the buffer solution composed of NH4Cl and NH4OH, which statement is correct?

How would you increase the pH of an acidic buffer solution?

In what scenario does a buffer solution experience maximum capacity to resist pH changes?

What is the impact of a common ion on the pH of a buffer solution?

What is formed when iron(III) ions react with thiocyanate ions?

Which of the following solutions would conduct electricity effectively?

What term refers to the equilibrium established between ionized and unionized molecules in a solution?

Which of the following is a strong electrolyte?

If the concentration of reactants in an equilibrium system is increased, what will happen to the equilibrium position?

What effect does increasing temperature have on the equilibrium constant (K) of an endothermic reaction?

Which of the following statements about weak acids is true?

What would happen to the yield of NH₃ if the pressure is increased in the Haber process?

In which reaction does the equilibrium constant decrease with an increase in temperature?

What must be true about a strong electrolyte in an aqueous solution?

Which of the following ions is produced by the ionization of hydrochloric acid in water?

What is the main consequence of a catalyst in a chemical reaction at equilibrium?

In an ionic equilibrium involving a weak acid, which species exists predominantly at equilibrium?

What is the primary role of water in the dissociation of ionic compounds?