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Which reaction shown will have the highest concentration of products at equilibrium?


A) Which reaction shown will have the highest concentration of products at equilibrium? A) B) C) D) E)
B) Which reaction shown will have the highest concentration of products at equilibrium? A) B) C) D) E)
C) Which reaction shown will have the highest concentration of products at equilibrium? A) B) C) D) E)
D) Which reaction shown will have the highest concentration of products at equilibrium? A) B) C) D) E)
E) Which reaction shown will have the highest concentration of products at equilibrium? A) B) C) D) E)

F) A) and C)
G) A) and E)

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Which is the correct equilibrium constant expression for the following reaction? 2BrCl3(g) Which is the correct equilibrium constant expression for the following reaction? 2BrCl<sub>3</sub>(g) Br<sub>2</sub>(g) + 3Cl<sub>2</sub>(g) A) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]/[BrCl<sub>3</sub>] B) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]<sup>5</sup>/[BrCl<sub>3</sub>]<sup>2</sup> C) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]<sup>3</sup>/[BrCl<sub>3</sub>]<sup>2</sup> D) K<sub>c</sub> = [BrCl<sub>3</sub>]<sup>2</sup>/([Br<sub>2</sub>] × [Cl<sub>2</sub>]3) E) K<sub>c</sub> = 2[BrCl<sub>3</sub>]<sup><sub>2</sub></sup>/([Br<sup>2</sup>] × 3[Cl2]<sup>3</sup>) Br2(g) + 3Cl2(g)


A) Kc = [Br2] [Cl2]/[BrCl3]
B) Kc = [Br2] [Cl2]5/[BrCl3]2
C) Kc = [Br2] [Cl2]3/[BrCl3]2
D) Kc = [BrCl3]2/([Br2] × [Cl2]3)
E) Kc = 2[BrCl3]2/([Br2] × 3[Cl2]3)

F) D) and E)
G) None of the above

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During a chemical reaction, what defines when the concentrations of the reactants and products reach a constant level?


A) Elementary process
B) Reversible reaction
C) Rate law
D) Rate constant
E) Equilibrium

F) A) and C)
G) A) and E)

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If, in a particular process, reactants are able to form products, and products are also able to form reactants, then this process may be described as


A) a reversible process.
B) an elementary process.
C) at equilibrium.
D) forbidden.
E) a forward process.

F) B) and E)
G) B) and C)

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The reaction system POBr3(g) The reaction system POBr<sub>3</sub>(g) POBr(g) + Br<sub>2</sub>(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container? A) POBr will be consumed in order to establish a new equilibrium. B) The partial pressures of POBr<sub>3</sub> and POBr will remain steady while the partial pressure of bromine increases. C) The partial pressure of bromine will increase while the partial pressure of POBr decreases. D) The partial pressure of bromine remains steady while the partial pressures of POBr<sub>3</sub> and POBr increase. E) The forward reaction will proceed to establish equilibrium. POBr(g) + Br2(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?


A) POBr will be consumed in order to establish a new equilibrium.
B) The partial pressures of POBr3 and POBr will remain steady while the partial pressure of bromine increases.
C) The partial pressure of bromine will increase while the partial pressure of POBr decreases.
D) The partial pressure of bromine remains steady while the partial pressures of POBr3 and POBr increase.
E) The forward reaction will proceed to establish equilibrium.

F) A) and D)
G) A) and E)

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For the reaction 2X(g) + Y(g) For the reaction 2X(g) + Y(g) 2Z(g) , K = 1.00 ×10<sup>3</sup> at 500 K.If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z? A) 2.2 M B) 3.2 M C) 3.5 M D) 4.5 M E) 7.1 M 2Z(g) , K = 1.00 ×103 at 500 K.If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?


A) 2.2 M
B) 3.2 M
C) 3.5 M
D) 4.5 M
E) 7.1 M

F) B) and D)
G) B) and E)

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Which is the correct equilibrium constant expression for the following reaction? 2C6H6(g) + 15O2(g) Which is the correct equilibrium constant expression for the following reaction? 2C<sub>6</sub>H<sub>6</sub>(g) + 15O<sub>2</sub>(g) 12CO₂(g) + 6H₂O(g) A) B) C) D) E) 12CO₂(g) + 6H₂O(g)


A) Which is the correct equilibrium constant expression for the following reaction? 2C<sub>6</sub>H<sub>6</sub>(g) + 15O<sub>2</sub>(g) 12CO₂(g) + 6H₂O(g) A) B) C) D) E)
B) Which is the correct equilibrium constant expression for the following reaction? 2C<sub>6</sub>H<sub>6</sub>(g) + 15O<sub>2</sub>(g) 12CO₂(g) + 6H₂O(g) A) B) C) D) E)
C) Which is the correct equilibrium constant expression for the following reaction? 2C<sub>6</sub>H<sub>6</sub>(g) + 15O<sub>2</sub>(g) 12CO₂(g) + 6H₂O(g) A) B) C) D) E)
D) Which is the correct equilibrium constant expression for the following reaction? 2C<sub>6</sub>H<sub>6</sub>(g) + 15O<sub>2</sub>(g) 12CO₂(g) + 6H₂O(g) A) B) C) D) E)
E) Which is the correct equilibrium constant expression for the following reaction? 2C<sub>6</sub>H<sub>6</sub>(g) + 15O<sub>2</sub>(g) 12CO₂(g) + 6H₂O(g) A) B) C) D) E)

F) C) and D)
G) A) and E)

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At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.

A) True
B) False

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A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H<sub>2</sub>(g) + N<sub>2</sub>(g) 2NH<sub>3</sub>(g) A) There will be no effect. B) More ammonia will be produced at the expense of hydrogen and nitrogen. C) Hydrogen and nitrogen will be produced at the expense of ammonia. D) The equilibrium constant will increase. E) The equilibrium constant will decrease. 2NH3(g)


A) There will be no effect.
B) More ammonia will be produced at the expense of hydrogen and nitrogen.
C) Hydrogen and nitrogen will be produced at the expense of ammonia.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.

F) A) and E)
G) B) and E)

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Which reaction shown will have the highest concentration of reactants at equilibrium?


A) Which reaction shown will have the highest concentration of reactants at equilibrium? A) B) C) D) E)
B) Which reaction shown will have the highest concentration of reactants at equilibrium? A) B) C) D) E)
C) Which reaction shown will have the highest concentration of reactants at equilibrium? A) B) C) D) E)
D) Which reaction shown will have the highest concentration of reactants at equilibrium? A) B) C) D) E)
E) Which reaction shown will have the highest concentration of reactants at equilibrium? A) B) C) D) E)

F) B) and E)
G) A) and D)

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