7234066
Frage 1
Frage
At equilibrium, __________.
Antworten
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A) all chemical reactions have ceased
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B) the rates of the forward and reverse reactions are equal
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C) the rate constants of the forward and reverse reactions are equal
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D) the value of the equilibrium constant is 1
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E) the limiting reagent has been consumed
Frage 2
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Which one of the following will change the value of an equilibrium constant?
Antworten
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A) changing temperature
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B) adding other substances that do not react with any of the species involved in the equilibrium
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C) varying the initial concentrations of reactants
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D) varying the initial concentrations of products
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E) changing the volume of the reaction vessel
Frage 3
Frage
The equilibrium-constant expression depends on the __________ of the reaction.
Antworten
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A) stoichiometry
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B) mechanism
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C) stoichiometry and mechanism
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D) the quantities of reactants and products initially present
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E) temperature
Frage 4
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The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is __________.
(1) SO2 (g) + (1/2) O2 (g) --> SO3 (g)
(2) 2SO3 (g) --> 2SO2 (g) + O2 (g)
Antworten
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A) K2
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B) 2K
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C) 1/2K
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D) 1/K2
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E) -K2
Frage 5
Frage
The value of Keq for the following reaction is 0.25:
SO2 (g) + NO2 (g) ---> SO3 (g) + NO (g)
The value of Keq at the same temperature for the reaction below is __________.
2SO2 (g) + 2NO2 (g) ---> 2SO3 (g) + 2NO (g)
Antworten
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A) 0.50
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B) 0.063
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C) 0.12
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D) 0.25
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E) 16
Frage 6
Frage
The Keq for the equilibrium below is 7.52 × 10-2 at 480.0°C.
2Cl2 (g) + 2H2O (g) --> 4HCl (g) + O2 (g)
What is the value of Keq at this temperature for the following reaction?
4HCl (g) + O2 (g) --> 2Cl2 (g) + 2H2O (g)
Antworten
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A) 0.0752
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B) -0.0752
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C) 13.3
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D) 5.66 × 10-3
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E) 0.150
Frage 7
Frage
Given the following reaction at equilibrium, if Kc = 1.90 × 1019 at 25.0°C, Kp = __________.
H2 (g) + Br2 (g) ---> 2 HBr (g)
Antworten
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A) 5.26 × 10-20
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B) 1.56 × 104
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C) 6.44 × 105
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D) 1.90 × 1019
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E) none of the above
Frage 8
Frage
The equilibrium constant for the gas phase reaction
N2 (g) + 3H2 (g) --> 2NH3 (g)
is Keq = 4.34 × 10-3 at 300°C. At equilibrium, __________.
Antworten
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A) products predominate
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B) reactants predominate
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C) roughly equal amounts of products and reactants are present
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D) only products are present
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E) only reactants are present
Frage 9
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The equilibrium constant for the gas phase reaction
2SO2 (g) + O2 (g) --> 2SO3 (g)
is Keq = 2.80 × 102 at 999 K. At equilibrium, __________.
Antworten
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A) products predominate
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B) reactants predominate
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C) roughly equal amounts of products and reactants are present
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D) only products are present
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E) only reactants are present
Frage 10
Frage
Consider the following equilibrium.
2SO2 (g) + O2 (g) --> 2SO3 (g)
The equilibrium cannot be established when __________ is/are placed in a 1.0-L container.
Antworten
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A) 0.25 mol SO2 (g) and 0.25 mol O2 (g)
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B) 0.75 mol SO2 (g)
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C) 0.25 mol of SO2 (g) and 0.25 mol of SO3 (g)
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D) 0.50 mol O2 (g) and 0.50 mol SO3 (g)
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E) 1.0 mol SO3 (g)
Frage 11
Frage
At 400 K, the equilibrium constant for the reaction
Br2 (g) + Cl2 (g) --> 2BrCl (g)
is Kp = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br2 (g), 1.00 atm of Cl2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true.
Antworten
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A) The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values.
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B) The equilibrium partial pressure of Br2 will be greater than 1.00 atm.
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C) At equilibrium, the total pressure in the vessel will be less than the initial total pressure.
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D) The equilibrium partial pressure of BrCl (g) will be greater than 2.00 atm.
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E) The reaction will go to completion since there are equal amounts of Br2 and Cl2.
Frage 12
Frage
How is the reaction quotient used to determine whether a system is at equilibrium?
Antworten
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A) The reaction quotient must be satisfied for equilibrium to be achieved.
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B) At equilibrium, the reaction quotient is undefined.
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D) The reaction is at equilibrium when Q > Keq.
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E) The reaction is at equilibrium when Q = Keq.
Frage 13
Frage
Of the following equilibria, only __________ will shift to the right in response to a decrease in volume.
Antworten
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A) H2 (g) + Cl2 (g) ---> 2 HCl (g)
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B) 2 SO3 (g) ---> 2 SO2 (g) + O2 (g)
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C) N2 (g) + 3 H2 (g) ---> 2 NH3 (g)
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D) 2 Fe2O3 (s) ---> 4 Fe (s) + 3 O2 (g)
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E) 2HI (g) ---> H2 (g) + I2 (g)
Frage 14
Frage
The reaction below is exothermic:
2SO2 (g) + O2 (g) ---> 2SO3 (g)
Le Châtelier's Principle predicts that __________ will result in an increase in the number of moles of SO3 (g) in the reaction container.
Antworten
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A) increasing the pressure
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B) decreasing the pressure
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C) increasing the temperature
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D) removing some oxygen
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E) increasing the volume of the container
Frage 15
Frage
For the endothermic reaction
CaCO3 (s) --> CaO (s) + CO2 (g)
Le Châtelier's principle predicts that __________ will result in an increase in the number of moles of CO2.
Antworten
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A) increasing the temperature
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B) decreasing the temperature
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C) increasing the pressure
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D) removing some of the CaCO3 (s)
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E) none of the above
Frage 16
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In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle?
Antworten
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A) N2 (g) + 3H2 (g) 2NH3 (g)
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B) N2O4 (g) 2NO2 (g)
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C) N2 (g) + 2O2 (g) 2NO2 (g)
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D) 2N2 (g) + O2 (g) 2N2O (g)
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E) N2 (g) + O2 (g) 2NO (g)
Frage 17
Frage
Consider the following reaction at equilibrium:
2NH3 (g) ---> N2 (g) + 3H2 (g) ΔH° = +92.4 kJ
Le Châtelier's principle predicts that adding N2 (g) to the system at equilibrium will result in __________.
Antworten
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A) a decrease in the concentration of NH3 (g)
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B) a decrease in the concentration of H2 (g)
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C) an increase in the value of the equilibrium constant
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D) a lower partial pressure of N2
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E) removal of all of the H2 (g)
Frage 18
Frage
Consider the following reaction at equilibrium:
2NH3 (g) ----> N2 (g) + 3H2 (g)
Le Châtelier's principle predicts that the moles of H2 in the reaction container will increase with __________.
Antworten
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A) some removal of NH3 from the reaction vessel (V and T constant)
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B) a decrease in the total pressure (T constant)
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C) addition of some N2 to the reaction vessel (V and T constant)
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D) a decrease in the total volume of the reaction vessel (T constant)
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E) an increase in total pressure by the addition of helium gas (V and T constant)
Frage 19
Frage
Consider the following reaction at equilibrium:
2CO2 (g) ---> 2CO (g) + O2 (g) ΔH° = -514 kJ
Le Châtelier's principle predicts that adding O2 (g) to the reaction container will __________.
Antworten
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A) increase the partial pressure of CO (g) at equilibrium
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B) decrease the partial pressure of CO2 (g) at equilibrium
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C) increase the value of the equilibrium constant
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D) increase the partial pressure of CO2 (g) at equilibrium
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E) decrease the value of the equilibrium constant
Frage 20
Frage
Consider the following reaction at equilibrium:
2CO2 (g) ----> 2CO (g) + O2 (g) ΔH° = -514 kJ
Le Châtelier's principle predicts that an increase in temperature will __________.
Antworten
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A) increase the partial pressure of O2 (g)
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B) decrease the partial pressure of CO2 (g)
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C) decrease the value of the equilibrium constant
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D) increase the value of the equilibrium constant
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E) increase the partial pressure of CO
Frage 21
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Consider the following reaction at equilibrium:
C (s) + H2O (g) ----> CO (g) + H2 (g)
Which of the following conditions will increase the partial pressure of CO?
Antworten
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A) decreasing the partial pressure of H2O (g)
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B) removing H2O (g) from the system
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C) decreasing the volume of the reaction vessel
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D) decreasing the pressure in the reaction vessel
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E) increasing the amount of carbon in the system
Frage 22
Frage
Consider the following reaction at equilibrium.
2CO2 (g) ---> 2CO (g) + O2 (g) ΔH° = -514 kJ
Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________.
Antworten
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A) at high temperature and high pressure
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B) at high temperature and low pressure
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C) at low temperature and low pressure
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D) at low temperature and high pressure
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E) in the presence of solid carbon
Frage 23
Frage
Consider the following reaction at equilibrium:
2SO2 (g) + O2 (g) --> 2SO3 (g) ΔH° = -99 kJ
Le Châtelier's principle predicts that an increase in temperature will result in __________.
Antworten
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A) a decrease in the partial pressure of SO3
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B) a decrease in the partial pressure of SO2
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C) an increase in Keq
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D) no changes in equilibrium partial pressures
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E) the partial pressure of O2 will decrease
Frage 24
Frage
The effect of a catalyst on an equilibrium is to __________.
Antworten
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A) increase the rate of the forward reaction only
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B) increase the equilibrium constant so that products are favored
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C) slow the reverse reaction only
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D) increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture
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E) shift the equilibrium to the right
Frage 25
Frage
The value of Keq for the equilibrium
H2 (g) + I2 (g) ---> 2 HI (g)
is 794 at 25 °C. What is the value of Keq for the equilibrium below?
1/2 H2 (g) + 1/2 I2 (g) ---> HI (g)
Antworten
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A) 397
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B) 0.035
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C) 28
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D) 1588
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E) 0.0013
Frage 26
Frage
The value of Keq for the equilibrium
H2 (g) + I2 (g) ---> 2 HI (g)
is 794 at 25°C. At this temperature, what is the value of Keq for the equilibrium below?
HI (g) ---> 1/2 H2 (g) + 1/2 I2 (g)
Antworten
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A) 1588
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B) 28
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C) 397
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D) 0.035
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E) 0.0013
Frage 27
Frage
Given the following reaction:
CO (g) + 2H2(g) ---> CH3OH (g)
In an experiment, 0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. Keq at the temperature of the experiment is __________.
Antworten
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A) 2.80
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B) 0.357
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C) 14.5
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D) 17.5
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E) none of the above
Frage 28
Frage
At 200°C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103.
2NO (g) ---> N2 (g) + O2 (g)
A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is __________ atm.
Antworten
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A) 294
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B) 35.7
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C) 17.9
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D) 6.00
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E) 1.50 × 10-2
Frage 29
Frage
Given the following reaction at equilibrium, if Kc = 6.34 x 105 at 230.0°C, Kp = __________.
2NO (g) + O2 (g) ---> 2NO2 (g)
Antworten
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A) 3.67 × 10-2
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B) 1.53 × 104
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C) 6.44 × 105
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D) 2.61 × 106
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E) 2.62 × 107
Frage 30
Frage
Nitrosyl bromide decomposes according to the following equation.
2NOBr (g) ---> 2NO (g) + Br2 (g)
A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.36 mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium?
Antworten
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A) .28,.28
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B) .36,.18
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C) .28,.14
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D) .14,.23
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E) .36,.36
Frage 31
Frage
If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture contains mostly __________.
Antworten
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A) Reactants
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B) Products
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C) Neither, they are in equal amounts
Frage 32
Frage
The number obtained by substituting starting reactant and product concentrations into an equilibrium-constant expression is known as the __________.
Antworten
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A) Rate Constant
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B) Reaction Quotient
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C) Equilibrium Concentration
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D) Reaction Rate
Frage 33
Frage
The relationship between the concentrations of reactants and products of a system at equilibrium is given by the law of mass action.
Antworten
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True
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False
Frage 34
Frage
If a reaction is endothermic, __________ the reaction temperature results in an increase in K.
Antworten
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A) Increasing
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B) Decreasing
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C) Constant
Frage 35
Frage
For an exothermic reaction, increasing the reaction temperature results in a(an) __________ in K.
Antworten
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A) Increasing
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B) Decreasing
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C) Constant
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