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If the reaction quotient Q for a reaction is greater than the value of the equilibrium constant K for that reaction at a given temperature,________ must be converted to ________ for the system to reach equilibrium.

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The value of Keq for the equilibrium H2 (g) + I2 (g) The value of K<sub>eq</sub> for the equilibrium H<sub>2</sub> (g) + I<sub>2</sub> (g) 2HI (g) Is 794 at 25 °C.At this temperature,what is the value of K<sub>eq</sub> for the equilibrium below? HI (g) 1/2 H<sub>2</sub> (g) + 1/2 I<sub>2</sub> (g) A) 1588 B) 28 C) 397 D) 0.035 E) 0.0013 2HI (g) Is 794 at 25 °C.At this temperature,what is the value of Keq for the equilibrium below? HI (g) The value of K<sub>eq</sub> for the equilibrium H<sub>2</sub> (g) + I<sub>2</sub> (g) 2HI (g) Is 794 at 25 °C.At this temperature,what is the value of K<sub>eq</sub> for the equilibrium below? HI (g) 1/2 H<sub>2</sub> (g) + 1/2 I<sub>2</sub> (g) A) 1588 B) 28 C) 397 D) 0.035 E) 0.0013 1/2 H2 (g) + 1/2 I2 (g)


A) 1588
B) 28
C) 397
D) 0.035
E) 0.0013

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

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= 0.0198 at 721 K for the reaction 2HI (g) (g) + (g) In a particular experiment,the partial pressures of and at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm. A) 7.87 B) 27.0 C) 5.19 D) 0.103 E) 0.0106 = 0.0198 at 721 K for the reaction 2HI (g) = 0.0198 at 721 K for the reaction 2HI (g) (g) + (g) In a particular experiment,the partial pressures of and at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm. A) 7.87 B) 27.0 C) 5.19 D) 0.103 E) 0.0106 = 0.0198 at 721 K for the reaction 2HI (g) (g) + (g) In a particular experiment,the partial pressures of and at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm. A) 7.87 B) 27.0 C) 5.19 D) 0.103 E) 0.0106 (g) + = 0.0198 at 721 K for the reaction 2HI (g) (g) + (g) In a particular experiment,the partial pressures of and at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm. A) 7.87 B) 27.0 C) 5.19 D) 0.103 E) 0.0106 (g) In a particular experiment,the partial pressures of = 0.0198 at 721 K for the reaction 2HI (g) (g) + (g) In a particular experiment,the partial pressures of and at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm. A) 7.87 B) 27.0 C) 5.19 D) 0.103 E) 0.0106 and = 0.0198 at 721 K for the reaction 2HI (g) (g) + (g) In a particular experiment,the partial pressures of and at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm. A) 7.87 B) 27.0 C) 5.19 D) 0.103 E) 0.0106 at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm.


A) 7.87
B) 27.0
C) 5.19
D) 0.103
E) 0.0106

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

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In an experiment,0.42 mol of CO and 0.42 mol of H2 were placed in a 1.00-L reaction vessel to yield CH3OH.At equilibrium,there were 0.29 mol of CO remaining.Keq at the temperature of the experiment is ________.


A) 2.80
B) 17.5
C) 0.357
D) 14.5
E) none of the above

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

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The value of Keq for the equilibrium H2 (g) + I2 (g) The value of K<sub>eq</sub> for the equilibrium H<sub>2</sub> (g) + I<sub>2</sub> (g) 2HI (g) Is 54.0 at 427 °C.What is the value of K<sub>eq</sub> for the equilibrium below? HI (g) 1/2 H<sub>2</sub> (g) + 1/2 I<sub>2</sub>(g) A) 27 B) 7.35 C) 0.136 D) 2.92 × 10<sup>3</sup> E) 3.43 × 10<sup>-4</sup> 2HI (g) Is 54.0 at 427 °C.What is the value of Keq for the equilibrium below? HI (g) The value of K<sub>eq</sub> for the equilibrium H<sub>2</sub> (g) + I<sub>2</sub> (g) 2HI (g) Is 54.0 at 427 °C.What is the value of K<sub>eq</sub> for the equilibrium below? HI (g) 1/2 H<sub>2</sub> (g) + 1/2 I<sub>2</sub>(g) A) 27 B) 7.35 C) 0.136 D) 2.92 × 10<sup>3</sup> E) 3.43 × 10<sup>-4</sup> 1/2 H2 (g) + 1/2 I2(g)


A) 27
B) 7.35
C) 0.136
D) 2.92 × 103
E) 3.43 × 10-4

F) C) and D)
G) B) and C)

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Define the reaction quotient.

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The number obtained by substit...

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Dinitrogentetraoxide partially decomposes into nitrogen dioxide.A 1.00-L flask is charged with Dinitrogentetraoxide partially decomposes into nitrogen dioxide.A 1.00-L flask is charged with of N<sub>2</sub>O<sub>4</sub>.At equilibrium at 373 K,0.0055 mol of N<sub>2</sub>O<sub>4</sub> remains.K<sub>eq</sub> for this reaction is ________. A) 2.2 × 10<sup>-4</sup> B) 13 C) 0.22 D) 0.87 E) 0.022 of N2O4.At equilibrium at 373 K,0.0055 mol of N2O4 remains.Keq for this reaction is ________.


A) 2.2 × 10-4
B) 13
C) 0.22
D) 0.87
E) 0.022

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

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The equilibrium constant for the gas phase reaction 2SO2 (g) + O2 (g) The equilibrium constant for the gas phase reaction 2SO<sub>2</sub> (g) + O<sub>2</sub> (g) 2SO<sub>3</sub> (g) Is K<sub>eq</sub> = 2.80 × 10<sup>2</sup> at 999 K.At equilibrium,________. A) products predominate B) reactants predominate C) roughly equal amounts of products and reactants are present D) only products are present E) only reactants are present 2SO3 (g) Is Keq = 2.80 × 102 at 999 K.At equilibrium,________.


A) products predominate
B) reactants predominate
C) roughly equal amounts of products and reactants are present
D) only products are present
E) only reactants are present

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

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The effect of a catalyst on an equilibrium is to ________.


A) increase the rate of the forward reaction only
B) increase the equilibrium constant so that products are favored
C) slow the reverse reaction only
D) increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture
E) shift the equilibrium to the right

F) All of the above
G) None of the above

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At equilibrium,________.


A) all chemical reactions have ceased
B) the rates of the forward and reverse reactions are equal
C) the rate constants of the forward and reverse reactions are equal
D) the value of the equilibrium constant is 1
E) the limiting reagent has been consumed

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

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Fritz Haber was awarded the ________ Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen.


A) 1954
B) 1918
C) 1933
D) 1900
E) 1912

F) B) and D)
G) B) and C)

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Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) 2NO (g) + (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or .At equilibrium the flask contained of NOBr.How many moles of NO and ,respectively,are in the flask at equilibrium? A) 0.48, 0.24 B) 0.48, 0.48 C) 0.16, 0.08 D) 0.16, 0.16 E) 0.24, 0.42 2NO (g) + Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) 2NO (g) + (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or .At equilibrium the flask contained of NOBr.How many moles of NO and ,respectively,are in the flask at equilibrium? A) 0.48, 0.24 B) 0.48, 0.48 C) 0.16, 0.08 D) 0.16, 0.16 E) 0.24, 0.42 (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) 2NO (g) + (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or .At equilibrium the flask contained of NOBr.How many moles of NO and ,respectively,are in the flask at equilibrium? A) 0.48, 0.24 B) 0.48, 0.48 C) 0.16, 0.08 D) 0.16, 0.16 E) 0.24, 0.42 .At equilibrium the flask contained Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) 2NO (g) + (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or .At equilibrium the flask contained of NOBr.How many moles of NO and ,respectively,are in the flask at equilibrium? A) 0.48, 0.24 B) 0.48, 0.48 C) 0.16, 0.08 D) 0.16, 0.16 E) 0.24, 0.42 of NOBr.How many moles of NO and Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) 2NO (g) + (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or .At equilibrium the flask contained of NOBr.How many moles of NO and ,respectively,are in the flask at equilibrium? A) 0.48, 0.24 B) 0.48, 0.48 C) 0.16, 0.08 D) 0.16, 0.16 E) 0.24, 0.42 ,respectively,are in the flask at equilibrium?


A) 0.48, 0.24
B) 0.48, 0.48
C) 0.16, 0.08
D) 0.16, 0.16
E) 0.24, 0.42

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

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The equilibrium constant for the gas phase reaction 2NH3 (g) The equilibrium constant for the gas phase reaction 2NH<sub>3</sub> (g) N<sub>2</sub> (g) + 3H<sub>2</sub> (g) Is K<sub>eq</sub> = 230 at 300 °C.At equilibrium,________. A) products predominate B) reactants predominate C) roughly equal amounts of products and reactants are present D) only products are present E) only reactants are present N2 (g) + 3H2 (g) Is Keq = 230 at 300 °C.At equilibrium,________.


A) products predominate
B) reactants predominate
C) roughly equal amounts of products and reactants are present
D) only products are present
E) only reactants are present

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

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The Keq for the equilibrium below is 5.4 × 1013 at 480.0 °C. 2NO (g) + O2 (g) The K<sub>eq</sub> for the equilibrium below is 5.4 × 10<sup>13</sup> at 480.0 °C. 2NO (g) + O<sub>2</sub> (g) 2NO<sub>2</sub> (g) What is the value of K<sub>eq</sub> at this temperature for the following reaction? 2NO<sub>2</sub> (g) 2NO (g) + O<sub>2</sub> (g) A) 5.4 × 10<sup>-13</sup> B) 1.9 × 10<sup>-14</sup> C) 5.4 × 10<sup>13</sup> D) 5.66 × 10<sup>-3</sup> E) none of the above 2NO2 (g) What is the value of Keq at this temperature for the following reaction? 2NO2 (g) The K<sub>eq</sub> for the equilibrium below is 5.4 × 10<sup>13</sup> at 480.0 °C. 2NO (g) + O<sub>2</sub> (g) 2NO<sub>2</sub> (g) What is the value of K<sub>eq</sub> at this temperature for the following reaction? 2NO<sub>2</sub> (g) 2NO (g) + O<sub>2</sub> (g) A) 5.4 × 10<sup>-13</sup> B) 1.9 × 10<sup>-14</sup> C) 5.4 × 10<sup>13</sup> D) 5.66 × 10<sup>-3</sup> E) none of the above 2NO (g) + O2 (g)


A) 5.4 × 10-13
B) 1.9 × 10-14
C) 5.4 × 1013
D) 5.66 × 10-3
E) none of the above

F) D) and E)
G) All of the above

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What role did Karl Bosch play in development of the Haber-Bosch process?


A) He discovered the reaction conditions necessary for formation of ammonia.
B) He originally isolated ammonia from camel dung and found a method for purifying it.
C) Haber was working in his lab with his instructor at the time he worked out the process.
D) He developed the equipment necessary for industrial production of ammonia.
E) He was the German industrialist who financed the research done by Haber.

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

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If the value for the equilibrium constant is much less than 1,then the equilibrium mixture contains mostly ________.

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Le Châtelier's principle states that if a system at equilibrium is disturbed,then more reactants are produced.

A) True
B) False

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At 24°C,Kp = 0.080 for the equilibrium: NH4HS (s) At 24°C,K<sub>p</sub> = 0.080 for the equilibrium: NH<sub>4</sub>HS (s) NH<sub>3 </sub>(g) + H<sub>2</sub>S (g) A sample of solid NH<sub>4</sub>HS is placed in a closed vessel and allowed to equilibrate.Calculate the equilibrium partial pressure (atm) of ammonia,assuming that some solid NH<sub>4</sub>HS remains. A) 0.28 B) 0.080 C) 0.052 D) 0.0049 E) 3.8 NH3 (g) + H2S (g) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate.Calculate the equilibrium partial pressure (atm) of ammonia,assuming that some solid NH4HS remains.


A) 0.28
B) 0.080
C) 0.052
D) 0.0049
E) 3.8

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

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Given the following reaction at equilibrium at 300.0 K: NH4HS (s) Given the following reaction at equilibrium at 300.0 K: NH<sub>4</sub>HS (s) NH<sub>3</sub> (g) + H<sub>2</sub>S (g) If pNH<sub>3</sub> = pH<sub>2</sub>S = 0.105 atm,K<sub>p</sub> = ________. A) .0110 B) 4.99 × 10<sup>-4</sup> C) .105 D) .0821 E) 5.66 × 10<sup>-3</sup> NH3 (g) + H2S (g) If pNH3 = pH2S = 0.105 atm,Kp = ________.


A) .0110
B) 4.99 × 10-4
C) .105
D) .0821
E) 5.66 × 10-3

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

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Consider the following reaction at equilibrium. 2CO2 (g) Consider the following reaction at equilibrium. 2CO<sub>2</sub> (g) 2CO (g) + O<sub>2</sub> (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 ________. A) at high temperature and high pressure B) at high temperature and low pressure C) at low temperature and low pressure D) at low temperature and high pressure E) in the presence of solid carbon 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 ________.


A) at high temperature and high pressure
B) at high temperature and low pressure
C) at low temperature and low pressure
D) at low temperature and high pressure
E) in the presence of solid carbon

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

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