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Exam 14: Chemical Equilibrium

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Question 41

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Which of the following statements best describes the rate of the forward reaction as it approaches equilibrium?

A) The rate increases as equilibrium is approached.
B) The rate decreases as equilibrium is approached.
C) The rate remains constant.
D) The rate slows down, then increases, as equilibrium is approached.

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Question 42

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For an endothermic reaction, lowering the temperature of the reaction will ________.

A) increase the amount of products
B) decrease the amount of reactants
C) decrease the amount of products
D) both A and B

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Question 43

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If the reaction vessel is expanded, this will ________. CH₄ (g) + 2O₂ (g) CO₂ (g) + 2H₂O (g)

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

Removing product will ________. 2SO₂ (g) + O₂ (g) 2SO₃ (g)

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

Calculate the equilibrium concentration of N₂ for the following reaction. + The equilibrium constant Keq is 0.055 and the concentrations of and are 1.20 M and 0.225 M, respectively.

Match each reaction and its equilibrium concentrations with its corresponding equilibrium constant value. -N?O₅ (g) 2 O? (g) + [N?O] = 0.50 M, [O?] = 1.0 M, [N?O₅] = 0.10 M

In an exothermic reaction, adding heat will ________.

Consider the reaction: C (s) + CO? (g) 2 CO (g) (endothermic) . Match each equilibrium change with its corresponding consequence. -decreasing the pressure

If the solubility of calcium fluoride is 2.0 × 10^-4 M, the solubility product value is ________.

Removing ozone as soon as it is formed will shift the equilibrium to the right. 3O₂ (g) ⇔ 2O₃ (g)

Write an expression for the equilibrium constant (Keq) for the following reaction. HCl (g) + H₂O (l) H₃O+ (aq)+ Cl- (aq)

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -2 SO₃ (g) + 2 CL₂ (g)

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

For an exothermic reaction, lowering the temperature of the reaction will ________.

Adding a catalyst to any reaction will always change the value of the equilibrium constant.

At equilibrium, the amount of product present is always greater than the amount of reactant present.

The double arrow in a chemical reaction indicates that the equilibrium is established since the rate of the forward reaction is equal to the rate of the reverse reaction.

The equilibrium concentrations for the reaction at 300 K are [CL₂] = 0.75 M, [PCL₃] = 0.45 M, and [PCl5] = 0.73 M. The value of Keq is ________. CL₂ (g) + PCL₃ (g) PCl5 (g)