FiltersDone

Question type

Essay

Multiple Choice

Short Answer

True False

Matching

Exam 14: Chemical Equilibrium

Show Answer

Share

---

All types

Filters

Study FlashcardsPractice ExamLearn

Question 1

Multiple Choice

Review LaterAdd Note

Review Later

The solubility of SrF₂ in water (given K_sp = 2.6 × 10^-9 ) is ________.

A) 4.3 × 10^{-4 M}
B) 1.2 × 10^{-4 M}
C) 7.6 × 10^{-5 M}
D) 8.7 × 10^{-4 M}

Correct Answer

verified

Show Answer

Question 2

Multiple Choice

Review LaterAdd Note

Review Later

For the reaction N₂ (g) + 2H₂ (g) ⇔ N₂H₄ (g) (endothermic) , what condition will increase the yield of product?

A) high temperature, high pressure
B) high temperature, low pressure
C) low temperature, high pressure
D) low temperature, low pressure

Correct Answer

verified

Show Answer

Question 3

Short Answer

Review LaterAdd Note

For the following exothermic reaction: CO + 3H₂ ⇔ CH₃OH predict the direction of the reaction if: a)temperature is decreased (concentrations remain the same). b)a catalyst is added (concentrations AND temperature remain the same). c)the concentration of H₂ is halved.

Consider the equation: CH₄ (g) + 2O₂ (g) ⇔ CO₂ (g) + 2H₂O (g) to answer the questions below. -Refer to the equilibrium shown above. If the reaction vessel is expanded, this will ________.

Write an expression for the equilibrium constant (K_eq)for the following reactions -C₆H₅NH₂ (aq)+ H₂O (l)⇔ C₆H₅NH₃⁺ (aq)+ OH^- (aq)

Consider the equation 2NH₃ (g) ⇔ N₂ (g) + 3H₂ (g) . Decreasing the concentration of ammonia gas will ________.

In an exothermic reaction, adding heat will ________.

Consider the equation N₂ (g) + 3H₂ (g) ⇔ 2NH₃ (g) . Removing ammonia as soon as it is formed will ________.

Consider the reaction: 2H₂S (g) + 3O₂ (g) ⇔ 2SO₂ (g) + 2H₂O (g) to answer the following questions. -Refer to the reaction shown above. Adding H₂O to the reaction vessel will ________.

Consider the reaction: C (s)+ CO₂ (g)⇔ 2 CO (g)(endothermic). Match each equilibrium change described in the questions with the corresponding consequence in the list below.

The equilibrium constant is equal to which of the following?

An equilibrium condition can be approached when the rate of a "forward" reaction slows down and the rate of a "reverse" reaction speeds up.

In the reaction Cl₂ (g)+ 3F₂ (g)⇔ 2ClF₃ (g), reducing the pressure will shift the equilibrium to the right.

Identify each of the equilibrium constant values in the questions as "Equilibrium lies to the right/products favored" or "Equilibrium lies to the left/reactants favored".

A reaction that favors products has a K_eq > 1.

Consider the reaction: FeCl₃ + KSCN ⇔ K₃[Fe(SCN) ₆] + 3KCl yellow colorless red colorless -Refer to the equilibrium shown above. Adding KSCN will ________.

If the solubility of copper(II) sulfate is 4.9 × 10^-3 M, the solubility product is ________.

Predict the effect of increasing pressure in each of the reactions in the questions by choosing the appropriate direction shift from the list below.

In the reaction PCl₅ ⇔ PCl₃ + Cl₂ at 500 K, the equilibrium concentrations of each species are [PCl₅] = 0.008 M, [PCl₃] = 0.02 M, and [Cl₂] = 0.02 M. The equilibrium constant value is 0.5.

If the value of the equilibrium constant for the forward reaction is 2.5 × 10³⁰, the value of the equilibrium constant for the reverse reaction is 4.0 × 10^-30.