Filters
Question type
Study Flashcards

Consider the equation A(aq) + 2B(aq) Consider the equation A(aq) + 2B(aq) 3C(aq) + 2D(aq) . 40.0 mL of 0.056 M A is mixed with 25.0 mL 0.108 M B. At equilibrium, the concentration of C is 0.0412 M. Calculate K. A) 0.029 B) 2.6 C) 0.0020 D) 1.9 × 10<sup>-4</sup> E) 0.013 3C(aq) + 2D(aq) . 40.0 mL of 0.056 M A is mixed with 25.0 mL 0.108 M B. At equilibrium, the concentration of C is 0.0412 M. Calculate K.


A) 0.029
B) 2.6
C) 0.0020
D) 1.9 × 10-4
E) 0.013

Correct Answer

verifed

verified

Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.​ A) ​ B) ​ C) ​ D) ​ E) ​ 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.​


A) ​ Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.​ A) ​ B) ​ C) ​ D) ​ E) ​
B) ​ Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.​ A) ​ B) ​ C) ​ D) ​ E) ​
C) ​ Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.​ A) ​ B) ​ C) ​ D) ​ E) ​
D) ​ Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.​ A) ​ B) ​ C) ​ D) ​ E) ​
E) ​ Consider the following chemical reaction involving a pure solid sample A that yields products B and C: 3A(s) 3B(g) + 2C(g) Identify the equilibrium expression of the reaction.​ A) ​ B) ​ C) ​ D) ​ E) ​

Correct Answer

verifed

verified

Which of the following statements concerning equilibrium is not true?


A) A system that is disturbed from an equilibrium condition responds in such a way as to restore equilibrium.
B) The value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained.
C) Equilibrium in molecular systems is dynamic, with two opposing processes balancing one another.
D) The equilibrium constant is independent of temperature.
E) A system moves spontaneously toward a state of equilibrium.

Correct Answer

verifed

verified

Which of the following statements is false?


A) Decreasing the volume of the container shifts the equilibrium to form more PCl5.
B) Removing PCl5 from the container shifts the equilibrium to form more PCl3.
C) Adding PCl3 to the container shifts the equilibrium to form more PCl5.
D) Increasing the temperature shifts the equilibrium to form more PCl3.

Correct Answer

verifed

verified

In the reaction P4(g)In the reaction P<sub>4</sub>(g) 2P<sub>2</sub>(g)K<sub>p</sub> = 0.500 atm at 1052°C. In an experiment, P<sub>4</sub>(g) is initially placed into a container at 1052°C. The total pressure of the equilibrium mixture of P<sub>4</sub>(g) and P<sub>2</sub>(g) is 6.00 atm. Calculate the equilibrium pressures of P<sub>4</sub>(g) and P<sub>2</sub>(g). Calculate the fraction (by moles) of P<sub>4</sub>(g) that has dissociated to reach equilibrium. 2P2(g)Kp = 0.500 atm at 1052°C. In an experiment, P4(g) is initially placed into a container at 1052°C. The total pressure of the equilibrium mixture of P4(g) and P2(g) is 6.00 atm. Calculate the equilibrium pressures of P4(g) and P2(g). Calculate the fraction (by moles) of P4(g) that has dissociated to reach equilibrium.

Correct Answer

verifed

verified

Pressure of P4 = 4.50...

View Answer

Consider the equation 2A(g) Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10<sup>4</sup>.Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will A) have no effect. B) cause [A] to increase. C) cause [B] to increase. D) cannot be determined E) none of these 2B(g) + C(g) . At a particular temperature, K = 1.6 × 104.Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will


A) have no effect.
B) cause [A] to increase.
C) cause [B] to increase.
D) cannot be determined
E) none of these

Correct Answer

verifed

verified

Write the equilibrium constant expression for the following reaction: CaCO3(s) Write the equilibrium constant expression for the following reaction: CaCO<sub>3</sub>(s) CaO(s) + CO<sub>2</sub>(g) CaO(s) + CO2(g)

Correct Answer

verifed

verified

Consider the equation 2A(g) Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10<sup>4</sup>. -Addition of chemical B to an equilibrium mixture of the above will A) cause [A] to increase. B) have no effect. C) cause [C] to increase. D) cannot be determined E) none of these 2B(g) + C(g) . At a particular temperature, K = 1.6 × 104. -Addition of chemical B to an equilibrium mixture of the above will


A) cause [A] to increase.
B) have no effect.
C) cause [C] to increase.
D) cannot be determined
E) none of these

Correct Answer

verifed

verified

The value of the equilibrium constant K is dependent on: I.the temperature of the system. II.the nature of the reactants and products. III.the concentration of the reactants. IV.the concentration of the products.


A) I and II only
B) III and IV only
C) II and III only
D) three of these
E) none of these

Correct Answer

verifed

verified

Consider the following reaction, which is involved in the catalytic destruction of ozone by chlorine atoms. ClO(g) + O3(g) Consider the following reaction, which is involved in the catalytic destruction of ozone by chlorine atoms. ClO(g) + O<sub>3</sub>(g) Cl(g) + 2O<sub>2</sub>(g) K<sub>p</sub> = 2.5 × 10<sup>6</sup> atm at 25° C. In an experiment at 25° C, ClO(g) at 1.0 × 10<sup>-3</sup> atm was mixed with O<sub>3</sub>(g) at 2.0 ×10<sup>-5</sup> atm in a rigid vessel. Calculate the equilibrium pressure of O<sub>3</sub>(g) and O<sub>2</sub>(g). Cl(g) + 2O2(g) Kp = 2.5 × 106 atm at 25° C. In an experiment at 25° C, ClO(g) at 1.0 × 10-3 atm was mixed with O3(g) at 2.0 ×10-5 atm in a rigid vessel. Calculate the equilibrium pressure of O3(g) and O2(g).

Correct Answer

verifed

verified

For O3, 1.3...

View Answer

For the reaction 2H2(g) + O2(g) For the reaction 2H<sub>2</sub>(g) + O<sub>2</sub>(g) 2H<sub>2</sub>O(g) , what is the relationship between K and K<sub>p</sub> at temperature T? A) K<sub>p</sub> = K(RT) <sup>2</sup> B) K = K<sub>p</sub>(RT) C) K = K<sub>p</sub> D) K<sub>p</sub> = K(RT) E) K = K<sub>p</sub>(RT) <sup>2</sup> 2H2O(g) , what is the relationship between K and Kp at temperature T?


A) Kp = K(RT) 2
B) K = Kp(RT)
C) K = Kp
D) Kp = K(RT)
E) K = Kp(RT) 2

Correct Answer

verifed

verified

Consider the following equilibrium:N2(g) + 3H2(g) Consider the following equilibrium:N<sub>2</sub>(g) + 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g) with K = 2.3 × 10<sup>-6</sup>. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of NH<sub>3</sub>(g) . A) 3.7 × 10<sup>-3</sup> M B) 5.4 × 10<sup>-5</sup> M C) 7.3 × 10<sup>-3</sup> M D) 4.3 × 10<sup>-6</sup> M E) none of these 2NH3(g) with K = 2.3 × 10-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of NH3(g) .


A) 3.7 × 10-3 M
B) 5.4 × 10-5 M
C) 7.3 × 10-3 M
D) 4.3 × 10-6 M
E) none of these

Correct Answer

verifed

verified

For the hypothetical reactions 1 and 2, K1 = 102 and K2 = 10-4. 1) A2(g) + B2(g) For the hypothetical reactions 1 and 2, K<sub>1</sub> = 10<sup>2</sup> and K<sub>2</sub> = 10<sup>-4</sup>. 1) A<sub>2</sub>(g) + B<sub>2</sub>(g) 2AB(g) 2) 2A<sub>2</sub>(g) + C<sub>2</sub>(g) 2A<sub>2</sub>C(g) 3) A<sub>2</sub>C(g) + B<sub>2</sub>(g) 2AB(g) + (1/2) C<sub>2</sub>(g) What is the value for K for reaction 3? A) 10<sup>-2</sup> B) 10<sup>4</sup> C) 10<sup>6</sup> D) 10<sup>2</sup> E) 10<sup>-4</sup> 2AB(g) 2) 2A2(g) + C2(g) For the hypothetical reactions 1 and 2, K<sub>1</sub> = 10<sup>2</sup> and K<sub>2</sub> = 10<sup>-4</sup>. 1) A<sub>2</sub>(g) + B<sub>2</sub>(g) 2AB(g) 2) 2A<sub>2</sub>(g) + C<sub>2</sub>(g) 2A<sub>2</sub>C(g) 3) A<sub>2</sub>C(g) + B<sub>2</sub>(g) 2AB(g) + (1/2) C<sub>2</sub>(g) What is the value for K for reaction 3? A) 10<sup>-2</sup> B) 10<sup>4</sup> C) 10<sup>6</sup> D) 10<sup>2</sup> E) 10<sup>-4</sup>2A2C(g) 3) A2C(g) + B2(g) For the hypothetical reactions 1 and 2, K<sub>1</sub> = 10<sup>2</sup> and K<sub>2</sub> = 10<sup>-4</sup>. 1) A<sub>2</sub>(g) + B<sub>2</sub>(g) 2AB(g) 2) 2A<sub>2</sub>(g) + C<sub>2</sub>(g) 2A<sub>2</sub>C(g) 3) A<sub>2</sub>C(g) + B<sub>2</sub>(g) 2AB(g) + (1/2) C<sub>2</sub>(g) What is the value for K for reaction 3? A) 10<sup>-2</sup> B) 10<sup>4</sup> C) 10<sup>6</sup> D) 10<sup>2</sup> E) 10<sup>-4</sup>2AB(g) + (1/2) C2(g) What is the value for K for reaction 3?


A) 10-2
B) 104
C) 106
D) 102
E) 10-4

Correct Answer

verifed

verified

Consider the equation 2A(g) Consider the equation 2A(g) 2B(g) + C(g) . At a particular temperature, K = 1.6 × 10<sup>4</sup>.At a higher temperature, K = 1.8 × 10<sup>-5</sup>. If you start with 2.0 M of chemical A, calculate the equilibrium concentration of chemical C. A) 2.6 × 10<sup>-2</sup> M B) 6.0 × 10<sup>-3</sup> M C) 1.0 M D) 2.1 × 10<sup>-2</sup> M E) none of these 2B(g) + C(g) . At a particular temperature, K = 1.6 × 104.At a higher temperature, K = 1.8 × 10-5. If you start with 2.0 M of chemical A, calculate the equilibrium concentration of chemical C.


A) 2.6 × 10-2 M
B) 6.0 × 10-3 M
C) 1.0 M
D) 2.1 × 10-2 M
E) none of these

Correct Answer

verifed

verified

For the reaction below, Kp = 1.16 at 890.°C. CaCO3(s) ⇌ CaO(s) + CO2(g) If a 22.0-g sample of CaCO3 is put into a 10.4-L container and heated to 890.°C, what percent of the CaCO3 will react to reach equilibrium?


A) 12.6%
B) 25.3%
C) 57.5%
D) 100.%
E) 54.9%

Correct Answer

verifed

verified

When the substances in the equation below are at equilibrium at pressure P and temperature T, how can the equilibrium be shifted to favor the products? CuO(s) + H2(g) When the substances in the equation below are at equilibrium at pressure P and temperature T, how can the equilibrium be shifted to favor the products? CuO(s) + H<sub>2</sub>(g) Cu(s) + H<sub>2</sub>O(g) Change in enthalpy = -2.0 kJ. A) Increase the pressure by adding an inert gas such as nitrogen. B) Allow some gas to escape at constant pressure and temperature. C) Decrease the temperature. D) Increase the pressure by means of a moving piston at constant temperature. E) Add a catalyst. Cu(s) + H2O(g) Change in enthalpy = -2.0 kJ.


A) Increase the pressure by adding an inert gas such as nitrogen.
B) Allow some gas to escape at constant pressure and temperature.
C) Decrease the temperature.
D) Increase the pressure by means of a moving piston at constant temperature.
E) Add a catalyst.

Correct Answer

verifed

verified

Consider the following equilibrium:N2(g) + 3H2(g) Consider the following equilibrium:N<sub>2</sub>(g) + 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g) with K = 2.3 × 10<sup>-6</sup>. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of H<sub>2</sub>. A) 0.5 M B) 1.0 M C) 2.5 M D) 2.0 M E) 1.5 M 2NH3(g) with K = 2.3 × 10-6. 1.00 mol each of all reactants and products is placed in a 1.00-L container. -Calculate the equilibrium concentration of H2.


A) 0.5 M
B) 1.0 M
C) 2.5 M
D) 2.0 M
E) 1.5 M

Correct Answer

verifed

verified

Consider the decomposition of hydrazine as shown below.N2H4(g) Consider the decomposition of hydrazine as shown below.N<sub>2</sub>H<sub>4</sub>(g) 2H<sub>2</sub>(g) + N<sub>2</sub>(g) At a certain temperature, K<sub>p</sub> = 2.5 × 10<sup>3</sup>. When pure hydrazine is placed in an otherwise empty vessel at this temperature, equilibrium is reached after 30.0% of the hydrazine has decomposed. Calculate the partial pressure of hydrogen gas at equilibrium. A) 76 atm B) 5776 atm C) 54 atm D) 127 atm E) none of these 2H2(g) + N2(g) At a certain temperature, Kp = 2.5 × 103. When pure hydrazine is placed in an otherwise empty vessel at this temperature, equilibrium is reached after 30.0% of the hydrazine has decomposed. Calculate the partial pressure of hydrogen gas at equilibrium.


A) 76 atm
B) 5776 atm
C) 54 atm
D) 127 atm
E) none of these

Correct Answer

verifed

verified

Showing 61 - 78 of 78

Related Exams

Exam 2

Atoms, Molecules, and Ions

66 Questions

Exam 3

Stoichiometry

105 Questions

Exam 4

Types of Chemical Reactions and Solution Stoichiometry

98 Questions

Exam 5

Gases

118 Questions

Exam 7

Acids and Bases

126 Questions

Exam 8

Applications of Aqueous Equilibria

177 Questions

Exam 9

Energy, Enthalpy, and Thermochemistry

86 Questions

Exam 10

Spontaneity, Entropy, and Free Energy

143 Questions

Exam 11

Electrochemistry

90 Questions

Exam 12

Quantum Mechanics and Atomic Theory

125 Questions

Exam 13

Bonding: General Concepts

136 Questions

Exam 14

Covalent Bonding: Orbitals

81 Questions

Exam 15

Chemical Kinetics

124 Questions

Exam 16

Liquids and Solids

111 Questions

Exam 17

Properties of Solutions

105 Questions

Exam 18

The Representative Elements

127 Questions

Exam 19

Transition Metals and Coordination Chemistry

96 Questions

Exam 20

The Nucleus: a Chemists View

73 Questions

Exam 21

Organic and Biochemical Molecules

123 Questions

Show Answer