Filters
Question type
Study Flashcards

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) C) and D)
G) A) and B)

Correct Answer

verifed

verified

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) A) and D)

Correct Answer

verifed

verified

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) C) and D)
G) A) and B)

Correct Answer

verifed

verified

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

Correct Answer

verifed

verified

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 B)
G) B) and E)

Correct Answer

verifed

verified

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

Correct Answer

verifed

verified

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) A) and B)
G) A) and C)

Correct Answer

verifed

verified

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) All of the above

Correct Answer

verifed

verified

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

A) True
B) False

Correct Answer

verifed

verified

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) None of the above
G) B) and E)

Correct Answer

verifed

verified

Showing 21 - 30 of 30

Related Exams

Exam 1

Atoms and Elements

50 Questions

Exam 2

Electrons and the Periodic Table

107 Questions

Exam 3

Compounds and Chemical Bonds

63 Questions

Exam 4

How Chemists Use Numbers

43 Questions

Exam 5

The Mole and Chemical Formulas

60 Questions

Exam 6

Molecular Shape

71 Questions

Exam 7

Solids, Liquids, and Phase Changes

58 Questions

Exam 8

Gases

60 Questions

Exam 9

Physical Properties of Solutions

62 Questions

Exam 10

Chemical Reactions and Chemical Equations

65 Questions

Exam 11

Using Balanced Chemical Equations

61 Questions

Exam 12

Acids and Bases

65 Questions

Exam 14

Organic Chemistry

46 Questions

Exam 15

Biochemistry

20 Questions

Exam 16

Nuclear Chemistry

38 Questions

Exam 17

Electrochemistry

30 Questions

Show Answer