Question 1

For the reaction Cu₂S(s)⇌ 2Cu⁺(aq)+ S^2-(aq),the equilibrium expression is:

Accepted Answer

The equilibrium expression should include the concentrations of the species involved in the reaction, raised to their stoichiometric coefficients in the balanced chemical equation. Here, the concentrations of CuS, CuS1P1+S1S1P0, and SS1P12-S1S1P0 are raised to the power of 1, 2, and 1, respectively. Therefore, option C is the correct equilibrium expression.

Question 2

Consider the reaction: 2 N₂O(g)⇌ O₂ (g)+ 2 N₂ (g).Which of the following will cause a shift in the equilibrium to the right? 1.Add more N₂O 2.Remove O₂ 3.Remove N₂

Accepted Answer

Adding more N₂O or removing O₂ or N₂ will shift the equilibrium to the right to produce more products according to Le Chatelier's principle.

Question 3

For the reaction S₂F₆ (g)⇌ 2SF₂ (g)+ F₂ (g),the equilibrium concentrations are as follows: [S₂F₆] = 0.000430 M,[SF₂] = 2.08 M,[F₂] = 1.32 M.The equilibrium constant is:

Accepted Answer

The equilibrium constant expression for the given reaction is: Kc = ([SF₂]²[F₂])/[S₂F₆] Substituting the given equilibrium concentrations, we get: Kc = (2.08)²(1.32)/(0.000430) = 1.33 × 10^14 Therefore, the best choice is option D.

Question 4

For the reaction S₂F₆ (g)⇌ 2SF₂ (g)+ F₂ (g),[SF₂] = 0.18 M,[F₂] = 0.54 M.The quilibrium constant is:

Accepted Answer

The equilibrium constant expression for the given reaction is: Kc=([SF₂]2[F₂])/([S₂][F₆]) Substituting the given values, we get: Kc=([0.18]2[0.54])/([1][1]) Kc=0.1458≈0.15 (rounded to two significant figures) Therefore, the correct answer is choice B.

Question 5

For the reaction Ag₂S(s)⇌ 2 Ag⁺ (aq)+ S^2- (aq),what happens to the equilibrium position if the amount of solid silver sulfide is doubled?

Accepted Answer

The equilibrium position is not affected by the amount of solid reactant or product, as solids do not appear in the equilibrium expression.

Question 6

Identify the equation for which K_eq = [Cu⁺]²[S^2-].

Accepted Answer

The answer of Identify the equation for which K_eq =...

Question 7

We have the following reaction at equilibrium in a flask, CaSO₄(s)⇌ Ca²⁺(aq)+ SO₄²⁺(aq) What will happen to [Ca²⁺] if additional CaSO₄ is added to the flask?

Accepted Answer

The answer of We have the following reaction at equilibrium...

Question 8

For the reaction 2 H₂O (l)⇌ 2H₂ (g)+ O₂ (g),the equilibrium expression is:

Accepted Answer

The equilibrium expression for the given reaction is: K_eq = [H₂]² [O₂] This is because the equilibrium constant expression always has the concentrations or partial pressures of the products raised to their stoichiometric coefficients divided by the concentrations or partial pressures of the reactants raised to their stoichiometric coefficients. In this case, the stoichiometric coefficients of the products and reactants are all 2.

Question 9

For the reaction Ag₂S(s)⇌ 2 Ag⁺ (aq)+ S^2- (aq),what happens to the equilibrium position if ammonium sulfate is added?

Accepted Answer

The addition of ammonium sulfate will not affect the equilibrium position of the reaction because it is a common ion effect. The ammonium ion will react with the hydroxide ion to form ammonium hydroxide, which will then dissociate to form ammonium ions and hydroxide ions. The hydroxide ions will then react with the silver ions to form silver hydroxide, which will precipitate out of solution. The removal of silver ions from solution will shift the equilibrium position to the left, but the addition of ammonium ions will shift the equilibrium position to the right. These two effects will cancel each other out, and the equilibrium position will remain the same.

Question 10

For the reaction Cu₂(s)⇌ 2Cu⁺(aq)+ S^2- (aq),the equilibrium concentrations are as follows: [Cu⁺ ] = 1.0 × 10^-5 M,[S^2-] = 1.0 × 10^-2 M.The equilibrium constant is:

Accepted Answer

The answer of For the reaction Cu₂(s)⇌ 2Cu⁺(aq)+ S^2- (aq),the...

Question 11

For the reaction Ag₂S(s)⇌ 2 Ag⁺ (aq)+ S^2- (aq),what happens to the equilibrium position if the amount of silver ion is halved?

Accepted Answer

Halving the concentration of silver ions will cause the equilibrium to shift to the right to produce more silver ions and restore equilibrium according to Le Chatelier's principle.

Question 12

For the reaction Ag₂S(s)⇌ 2 Ag⁺ (aq)+ S^2- (aq),what happens to the equilibrium position if aqueous ammonium sulfide is added?

Accepted Answer

Adding aqueous ammonium sulfide increases the concentration of S^2- ions, which shifts the equilibrium to the left according to Le Chatelier's principle to counteract the change.

Question 13

What must be TRUE for a reaction possessing a large equilibrium constant?

Accepted Answer

A large equilibrium constant (Kc) indicates that the forward reaction is favored over the reverse reaction, meaning that a greater amount of products are formed.

Question 14

For the reaction 2 A ⇌ B,the equilibrium concentrations are as follows: [A] = 0.056 M and [B] = 0.12 M.Calculate the equilibrium constant (K_eq )for the reaction.

Accepted Answer

The equilibrium constant (Kc) can be calculated by dividing the concentration of the products raised to their stoichiometric coefficients by the concentration of the reactants raised to their stoichiometric coefficients. For this reaction:
Kc = [B]^2/[A]^2 = (0.12)^2/(0.056)^2 = 38.48 ≈ 38 (rounded to 2 significant figures)

Therefore, the correct answer is D.

Question 15

For the reaction LiOH (s)⇌ Li⁺ (aq)+ OH^- (aq),K_eq = 4.6 × 10^-³,and the equilibrium concentration for hydroxide ion is [OH^-] = 0.042 M.What is [Li⁺] at equilibrium?

Accepted Answer

Using the equilibrium constant expression:
K_eq = [LiS_1+][OH^-]^1/[LiOH]
4.6 × 10^13 = [LiS_1+][0.042]^1/[LiOH]
Solving for [LiS_1+], we get:
[LiS_1+] = (4.6 × 10^13 × [LiOH])/0.042
Since the value of [LiOH] is not given, we cannot determine the exact numerical value of [LiS_1+], but we can see that it is directly proportional to [LiOH]. Therefore, as [OH^-] increases, [LiS_1+] also increases. The answer choice that reflects this relationship is A, 0.11 M.

Question 16

For the reaction Ag₂S(s)⇌ 2 Ag⁺ (aq)+ S^2- (aq),K_eq = 2.4 × 10^-4,and the equilibrium concentration of sulfide ion is [S^2-] = 0.0023 M..What is [Ag⁺] at equilibrium?

Accepted Answer

The answer of For the reaction Ag₂S(s)⇌ 2 Ag⁺ (aq)+...

Question 17

For the reaction Ag₂S(s)⇌ 2 Ag⁺ (aq)+ S^2- (aq),K_eq = 2.4 × 10^-4 and the equilibrium concentration of silver ion is [Ag⁺] = 2.5 × 10^-¹ M.What is [S^2-] at equilibrium?

Accepted Answer

The equilibrium constant expression for the given reaction is:K_eq = [Ag⁺]²[S^2-]Substituting the given values into the expression, we get:2.4 × 10^-4 = (2.5 × 10^-1)²[S^2-]Solving for [S^2-], we get:[S^2-] = 0.0038 MTherefore, the correct answer is A.

Question 18

Le Chatelier's Principle states that:

Accepted Answer

Le Chatelier's Principle states that when a chemical system at equilibrium is disturbed, the system will shift in order to minimize the effect of the disturbance and reestablish equilibrium. This can be seen when a system is subjected to changes in temperature, pressure, or concentration, as the system will adjust its reaction rate in order to counteract the change and maintain equilibrium.

Question 19

Consider the reaction: 2 N₂O(g)⇌ O₂ (g)+ 2 N₂ (g).Which of the following will cause a shift in the equilibrium to the left? 1.Remove N₂O 2.Remove O₂ 3.Add N₂

Accepted Answer

Removing N₂O or adding N₂ will shift the equilibrium to the left, according to Le Chatelier's principle.

Question 20

When writing the expression for an equilibrium constant,which type of substance IS included?

Accepted Answer

Equilibrium constant expressions only include gases and aqueous substances, as they can freely react and influence the reaction equilibrium. Solid and pure liquid substances are not included in the expression as their concentrations do not change during the reaction.

Quiz 15: Chemical Equilibrium

For the reaction Cu₂S(s) ⇌ 2Cu⁺(aq) + S^2-(aq) ,the equilibrium expression is:

Consider the reaction: 2 N₂O(g) ⇌ O₂ (g) + 2 N₂ (g) .Which of the following will cause a shift in the equilibrium to the right? 1.Add more N₂O 2.Remove O₂ 3.Remove N₂

For the reaction S₂F₆ (g) ⇌ 2SF₂ (g) + F₂ (g) ,the equilibrium concentrations are as follows: [S₂F₆] = 0.000430 M,[SF₂] = 2.08 M,[F₂] = 1.32 M.The equilibrium constant is:

For the reaction S₂F₆ (g) ⇌ 2SF₂ (g) + F₂ (g) ,[SF₂] = 0.18 M,[F₂] = 0.54 M.The quilibrium constant is:

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,what happens to the equilibrium position if the amount of solid silver sulfide is doubled?

Identify the equation for which K_eq = [Cu⁺]²[S^2-].

We have the following reaction at equilibrium in a flask, CaSO₄(s) ⇌ Ca²⁺(aq) + SO₄²⁺(aq) What will happen to [Ca²⁺] if additional CaSO₄ is added to the flask?

For the reaction 2 H₂O (l) ⇌ 2H₂ (g) + O₂ (g) ,the equilibrium expression is:

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,what happens to the equilibrium position if ammonium sulfate is added?

For the reaction Cu₂(s) ⇌ 2Cu⁺(aq) + S^2- (aq) ,the equilibrium concentrations are as follows: [Cu⁺ ] = 1.0 × 10^-5 M,[S^2-] = 1.0 × 10^-2 M.The equilibrium constant is:

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,what happens to the equilibrium position if the amount of silver ion is halved?

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,what happens to the equilibrium position if aqueous ammonium sulfide is added?

What must be TRUE for a reaction possessing a large equilibrium constant?

For the reaction 2 A ⇌ B,the equilibrium concentrations are as follows: [A] = 0.056 M and [B] = 0.12 M.Calculate the equilibrium constant (K_eq ) for the reaction.

For the reaction LiOH (s) ⇌ Li⁺ (aq) + OH^- (aq) ,K_eq = 4.6 × 10^-³,and the equilibrium concentration for hydroxide ion is [OH^-] = 0.042 M.What is [Li⁺] at equilibrium?

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,K_eq = 2.4 × 10^-4,and the equilibrium concentration of sulfide ion is [S^2-] = 0.0023 M..What is [Ag⁺] at equilibrium?

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,K_eq = 2.4 × 10^-4 and the equilibrium concentration of silver ion is [Ag⁺] = 2.5 × 10^-¹ M.What is [S^2-] at equilibrium?

Le Chatelier's Principle states that:

Consider the reaction: 2 N₂O(g) ⇌ O₂ (g) + 2 N₂ (g) .Which of the following will cause a shift in the equilibrium to the left? 1.Remove N₂O 2.Remove O₂ 3.Add N₂

When writing the expression for an equilibrium constant,which type of substance IS included?

Quiz 15: Chemical Equilibrium

For the reaction Cu2S(s) ⇌ 2Cu+(aq) + S2-(aq) ,the equilibrium expression is:

Consider the reaction: 2 N2O(g) ⇌ O2 (g) + 2 N2 (g) .Which of the following will cause a shift in the equilibrium to the right? 1.Add more N2O 2.Remove O2 3.Remove N2

For the reaction S2F6 (g) ⇌ 2SF2 (g) + F2 (g) ,the equilibrium concentrations are as follows: [S2F6] = 0.000430 M,[SF2] = 2.08 M,[F2] = 1.32 M.The equilibrium constant is:

For the reaction S2F6 (g) ⇌ 2SF2 (g) + F2 (g) ,[SF2] = 0.18 M,[F2] = 0.54 M.The quilibrium constant is:

For the reaction Ag2S(s) ⇌ 2 Ag+ (aq) + S2- (aq) ,what happens to the equilibrium position if the amount of solid silver sulfide is doubled?

Identify the equation for which Keq = [Cu+]2[S2-].

We have the following reaction at equilibrium in a flask, CaSO4(s) ⇌ Ca2+(aq) + SO42+(aq) What will happen to [Ca2+] if additional CaSO4 is added to the flask?

For the reaction 2 H2O (l) ⇌ 2H2 (g) + O2 (g) ,the equilibrium expression is:

For the reaction Ag2S(s) ⇌ 2 Ag+ (aq) + S2- (aq) ,what happens to the equilibrium position if ammonium sulfate is added?

For the reaction Cu2(s) ⇌ 2Cu+(aq) + S2- (aq) ,the equilibrium concentrations are as follows: [Cu+ ] = 1.0 × 10-5 M,[S2-] = 1.0 × 10-2 M.The equilibrium constant is:

For the reaction Ag2S(s) ⇌ 2 Ag+ (aq) + S2- (aq) ,what happens to the equilibrium position if the amount of silver ion is halved?

For the reaction Ag2S(s) ⇌ 2 Ag+ (aq) + S2- (aq) ,what happens to the equilibrium position if aqueous ammonium sulfide is added?

What must be TRUE for a reaction possessing a large equilibrium constant?

For the reaction 2 A ⇌ B,the equilibrium concentrations are as follows: [A] = 0.056 M and [B] = 0.12 M.Calculate the equilibrium constant (Keq ) for the reaction.

For the reaction LiOH (s) ⇌ Li+ (aq) + OH- (aq) ,Keq = 4.6 × 10-3,and the equilibrium concentration for hydroxide ion is [OH-] = 0.042 M.What is [Li+] at equilibrium?

For the reaction Ag2S(s) ⇌ 2 Ag+ (aq) + S2- (aq) ,Keq = 2.4 × 10-4,and the equilibrium concentration of sulfide ion is [S2-] = 0.0023 M..What is [Ag+] at equilibrium?

For the reaction Ag2S(s) ⇌ 2 Ag+ (aq) + S2- (aq) ,Keq = 2.4 × 10-4 and the equilibrium concentration of silver ion is [Ag+] = 2.5 × 10-1 M.What is [S2-] at equilibrium?

Le Chatelier's Principle states that:

Consider the reaction: 2 N2O(g) ⇌ O2 (g) + 2 N2 (g) .Which of the following will cause a shift in the equilibrium to the left? 1.Remove N2O 2.Remove O2 3.Add N2

When writing the expression for an equilibrium constant,which type of substance IS included?

For the reaction Cu₂S(s) ⇌ 2Cu⁺(aq) + S^2-(aq) ,the equilibrium expression is:

Consider the reaction: 2 N₂O(g) ⇌ O₂ (g) + 2 N₂ (g) .Which of the following will cause a shift in the equilibrium to the right? 1.Add more N₂O 2.Remove O₂ 3.Remove N₂

For the reaction S₂F₆ (g) ⇌ 2SF₂ (g) + F₂ (g) ,the equilibrium concentrations are as follows: [S₂F₆] = 0.000430 M,[SF₂] = 2.08 M,[F₂] = 1.32 M.The equilibrium constant is:

For the reaction S₂F₆ (g) ⇌ 2SF₂ (g) + F₂ (g) ,[SF₂] = 0.18 M,[F₂] = 0.54 M.The quilibrium constant is:

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,what happens to the equilibrium position if the amount of solid silver sulfide is doubled?

Identify the equation for which K_eq = [Cu⁺]²[S^2-].

We have the following reaction at equilibrium in a flask, CaSO₄(s) ⇌ Ca²⁺(aq) + SO₄²⁺(aq) What will happen to [Ca²⁺] if additional CaSO₄ is added to the flask?

For the reaction 2 H₂O (l) ⇌ 2H₂ (g) + O₂ (g) ,the equilibrium expression is:

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,what happens to the equilibrium position if ammonium sulfate is added?

For the reaction Cu₂(s) ⇌ 2Cu⁺(aq) + S^2- (aq) ,the equilibrium concentrations are as follows: [Cu⁺ ] = 1.0 × 10^-5 M,[S^2-] = 1.0 × 10^-2 M.The equilibrium constant is:

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,what happens to the equilibrium position if the amount of silver ion is halved?

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,what happens to the equilibrium position if aqueous ammonium sulfide is added?

For the reaction 2 A ⇌ B,the equilibrium concentrations are as follows: [A] = 0.056 M and [B] = 0.12 M.Calculate the equilibrium constant (K_eq ) for the reaction.

For the reaction LiOH (s) ⇌ Li⁺ (aq) + OH^- (aq) ,K_eq = 4.6 × 10^-³,and the equilibrium concentration for hydroxide ion is [OH^-] = 0.042 M.What is [Li⁺] at equilibrium?

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,K_eq = 2.4 × 10^-4,and the equilibrium concentration of sulfide ion is [S^2-] = 0.0023 M..What is [Ag⁺] at equilibrium?

For the reaction Ag₂S(s) ⇌ 2 Ag⁺ (aq) + S^2- (aq) ,K_eq = 2.4 × 10^-4 and the equilibrium concentration of silver ion is [Ag⁺] = 2.5 × 10^-¹ M.What is [S^2-] at equilibrium?

Consider the reaction: 2 N₂O(g) ⇌ O₂ (g) + 2 N₂ (g) .Which of the following will cause a shift in the equilibrium to the left? 1.Remove N₂O 2.Remove O₂ 3.Add N₂