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Consider the following gas-phase equilibrium reaction: Consider the following gas-phase equilibrium reaction: If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C,what is the concentration of NO when equilibrium is reached? If 1.0 mol of NO is introduced into a 1.0 L container at 2000°C,what is the concentration of NO when equilibrium is reached?

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[NO] = 1.0 \(\times\) 10-2 mol L-1

The reaction system CS2(g) + 4H2(g) The reaction system CS<sub>2</sub>(g) + 4H<sub>2</sub>(g) CH<sub>4</sub>(g) + 2H<sub>2</sub>S(g) Is at equilibrium.Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled? A) As equilibrium is reestablished,the partial pressure of carbon disulfide increases. B) As equilibrium is reestablished,the partial pressure of methane,CH<sub>4</sub>,decreases. C) As equilibrium is reestablished,the partial pressure of hydrogen decreases. D) As equilibrium is reestablished,the partial pressure of hydrogen sulfide decreases. E) As equilibrium is reestablished,all the partial pressures will decrease. CH4(g) + 2H2S(g) Is at equilibrium.Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?


A) As equilibrium is reestablished,the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished,the partial pressure of methane,CH4,decreases.
C) As equilibrium is reestablished,the partial pressure of hydrogen decreases.
D) As equilibrium is reestablished,the partial pressure of hydrogen sulfide decreases.
E) As equilibrium is reestablished,all the partial pressures will decrease.

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When a chemical system is at equilibrium,


A) the concentrations of the reactants are equal to the concentrations of the products.
B) the concentrations of the reactants and products have reached constant values.
C) the forward and reverse reactions have stopped.
D) the reaction quotient,Q,has reached a maximum.
E) the reaction quotient,Q,has reached a minimum.

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The reaction system POCl3(g) The reaction system POCl<sub>3</sub>(g) POCl(g) + Cl<sub>2</sub>(g) Is at equilibrium.Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%? A) POCl<sub>3</sub> will be consumed as equilibrium is established. B) POCl will be consumed as equilibrium is established. C) Chlorine will be consumed as equilibrium is established. D) The partial pressure of POCl will decrease while the partial pressure of Cl<sub>2</sub> increases as equilibrium is established. E) The volume will have to decrease before equilibrium can be reestablished. POCl(g) + Cl2(g) Is at equilibrium.Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%?


A) POCl3 will be consumed as equilibrium is established.
B) POCl will be consumed as equilibrium is established.
C) Chlorine will be consumed as equilibrium is established.
D) The partial pressure of POCl will decrease while the partial pressure of Cl2 increases as equilibrium is established.
E) The volume will have to decrease before equilibrium can be reestablished.

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Consider the equilibrium reaction: H2(g) + Br2(g) Consider the equilibrium reaction: H<sub>2</sub>(g) + Br<sub>2</sub>(g) 2HBr(g) Which of the following correctly describes the relationship between K<sub>c</sub> and K<sub>p</sub> for the reaction? A) K<sub>p</sub> = K<sub>c</sub> B) K<sub>p</sub> = (RT) K<sub>c</sub> C) K<sub>p</sub> = (RT) <sup>2</sup>K<sub>c</sub> D) K<sub>p</sub> = K<sub>c</sub>/RT E) K<sub>p</sub> = K<sub>c</sub>/(RT) <sup>2</sup> 2HBr(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?


A) Kp = Kc
B) Kp = (RT) Kc
C) Kp = (RT) 2Kc
D) Kp = Kc/RT
E) Kp = Kc/(RT) 2

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Magnesium hydroxide is used in several antacid formulations.When it is added to water it dissociates into magnesium and hydroxide ions. Mg(OH) 2(s) Magnesium hydroxide is used in several antacid formulations.When it is added to water it dissociates into magnesium and hydroxide ions. Mg(OH) <sub>2</sub>(s) Mg<sup>2+</sup>(aq) + 2OH<sup>-</sup>(aq) The equilibrium constant at 25°C is 8.9 \times 10<sup>-12</sup>.One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established.What happens to the solution if another 10 grams of Mg(OH) <sub>2</sub> are now added to the mixture? A) The hydroxide ion concentration will decrease. B) The hydroxide ion concentration will increase. C) The hydroxide ion concentration will be unchanged. D) The solution will become supersaturated. E) None of these conclusions is justified without additional information. Mg2+(aq) + 2OH-(aq) The equilibrium constant at 25°C is 8.9 ×\times 10-12.One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established.What happens to the solution if another 10 grams of Mg(OH) 2 are now added to the mixture?


A) The hydroxide ion concentration will decrease.
B) The hydroxide ion concentration will increase.
C) The hydroxide ion concentration will be unchanged.
D) The solution will become supersaturated.
E) None of these conclusions is justified without additional information.

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The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g) + Cl2(g) The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) A) 2.97 \times 10<sup>-4</sup> B) 1.72 \times 10<sup>-2</sup> C) 3.45 \times 10<sup>-2</sup> D) 1.31 \times 10<sup>-1</sup> E) > 1.00 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) A) 2.97 \times 10<sup>-4</sup> B) 1.72 \times 10<sup>-2</sup> C) 3.45 \times 10<sup>-2</sup> D) 1.31 \times 10<sup>-1</sup> E) > 1.00 The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) A) 2.97 \times 10<sup>-4</sup> B) 1.72 \times 10<sup>-2</sup> C) 3.45 \times 10<sup>-2</sup> D) 1.31 \times 10<sup>-1</sup> E) > 1.00 Br2(g) + The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) 2BrCl(g) What is the equilibrium constant for the following reaction? BrCl(g) Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) A) 2.97 \times 10<sup>-4</sup> B) 1.72 \times 10<sup>-2</sup> C) 3.45 \times 10<sup>-2</sup> D) 1.31 \times 10<sup>-1</sup> E) > 1.00 Cl2(g)


A) 2.97 ×\times 10-4
B) 1.72 ×\times 10-2
C) 3.45 ×\times 10-2
D) 1.31 ×\times 10-1
E) > 1.00

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If Q > K,more products need to be formed as the reaction proceeds to equilibrium.

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Once a reaction system reaches equilibrium,the concentrations of reactions and products no longer change.

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True

Write the mass-action expression,Qc,for the following chemical reaction. NO(g) + Write the mass-action expression,Q<sub>c</sub>,for the following chemical reaction. NO(g) + Br<sub>2</sub>(g) NOBr(g) A) B) C) D) E) Br2(g) Write the mass-action expression,Q<sub>c</sub>,for the following chemical reaction. NO(g) + Br<sub>2</sub>(g) NOBr(g) A) B) C) D) E) NOBr(g)


A)
Write the mass-action expression,Q<sub>c</sub>,for the following chemical reaction. NO(g) + Br<sub>2</sub>(g) NOBr(g) A) B) C) D) E)
B)
Write the mass-action expression,Q<sub>c</sub>,for the following chemical reaction. NO(g) + Br<sub>2</sub>(g) NOBr(g) A) B) C) D) E)
C)
Write the mass-action expression,Q<sub>c</sub>,for the following chemical reaction. NO(g) + Br<sub>2</sub>(g) NOBr(g) A) B) C) D) E)
D)
Write the mass-action expression,Q<sub>c</sub>,for the following chemical reaction. NO(g) + Br<sub>2</sub>(g) NOBr(g) A) B) C) D) E)
E)
Write the mass-action expression,Q<sub>c</sub>,for the following chemical reaction. NO(g) + Br<sub>2</sub>(g) NOBr(g) A) B) C) D) E)

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For a gas-phase equilibrium,a change in the pressure of any single reactant or product will change Kp.

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The equilibrium constant,Kc ,for the decomposition of COBr2 COBr2(g) The equilibrium constant,K<sub>c</sub> ,for the decomposition of COBr<sub>2</sub> <sub> </sub>COBr<sub>2</sub>(g) CO(g) + Br<sub>2</sub>(g) Is 0.190.What is K<sub>c</sub> for the following reaction? 2CO(g) + 2Br<sub>2</sub>(g) 2COBr<sub>2</sub>(g) A) 0.0361 B) 2.63 C) 5.62 D) 10.5 E) 27.7 CO(g) + Br2(g) Is 0.190.What is Kc for the following reaction? 2CO(g) + 2Br2(g) The equilibrium constant,K<sub>c</sub> ,for the decomposition of COBr<sub>2</sub> <sub> </sub>COBr<sub>2</sub>(g) CO(g) + Br<sub>2</sub>(g) Is 0.190.What is K<sub>c</sub> for the following reaction? 2CO(g) + 2Br<sub>2</sub>(g) 2COBr<sub>2</sub>(g) A) 0.0361 B) 2.63 C) 5.62 D) 10.5 E) 27.7 2COBr2(g)


A) 0.0361
B) 2.63
C) 5.62
D) 10.5
E) 27.7

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The reaction quotient,Qc,for a reaction has a value of 75 while the equilibrium constant,Kc,has a value of 195.Which of the following statements is accurate?


A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium.
D) The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium.
E) None of these statements is accurate.

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For a gas-phase equilibrium,a change in the pressure of any single reactant or product will affect the amounts of other substances involved in the equilibrium.

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A mixture 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr2 was 0.233 M.What is the value of Kc for this reaction? CO(g) + Br2(g) A mixture 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr<sub>2</sub> was 0.233 M.What is the value of K<sub>c</sub> for this reaction? CO(g) + Br<sub>2</sub>(g) COBr<sub>2</sub>(g) A) 5.23 B) 1.22 C) 1.165 D) 0.858 E) 0.191 COBr2(g)


A) 5.23
B) 1.22
C) 1.165
D) 0.858
E) 0.191

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The reaction quotient for a gas phase reaction has a value of 2000.If the number of moles of reactants in the reaction equation is equal to that of the products,which of the following statements is true?


A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) When the system is at equilibrium,the concentrations of the products will be much larger than the concentrations of the reactants.
D) The concentrations of the products are generally larger than the concentrations of the reactants.
E) None of these statements is true.

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D

Consider the equilibrium: Consider the equilibrium: Predict and explain how or whether the following actions would affect this equilibrium. a.adding more solid A b.lowering the temperature c.increasing the pressure on the system by reducing its volume d.adding helium gas to increase the total pressure Predict and explain how or whether the following actions would affect this equilibrium. a.adding more solid A b.lowering the temperature c.increasing the pressure on the system by reducing its volume d.adding helium gas to increase the total pressure

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a.No effect.Pure solids and liquids have...

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The following reaction is at equilibrium in a closed container. CuSO4.5H2O(s) The following reaction is at equilibrium in a closed container. CuSO<sub>4</sub>.5H<sub>2</sub>O(s) CuSO<sub>4</sub>(s) + 5H<sub>2</sub>O(g) Which,if any,of the following actions will lead to an increase in the pressure of H<sub>2</sub>O present at equilibrium? A) increasing the volume of the container B) decreasing the volume of the container C) adding a catalyst D) removing some solid CuSO<sub>4</sub> E) None of these choices is correct. CuSO4(s) + 5H2O(g) Which,if any,of the following actions will lead to an increase in the pressure of H2O present at equilibrium?


A) increasing the volume of the container
B) decreasing the volume of the container
C) adding a catalyst
D) removing some solid CuSO4
E) None of these choices is correct.

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At a certain temperature the reaction CO2(g) + H2(g) At a certain temperature the reaction CO<sub>2</sub>(g) + H<sub>2</sub>(g) CO(g) + H<sub>2</sub>O(g) Has K<sub>c</sub> = 2.50.If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established,what will be the concentration of carbon monoxide? A) 0.091 M B) 0.191 M C) 0.209 M D) 0.913 M E) 1.05 M CO(g) + H2O(g) Has Kc = 2.50.If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established,what will be the concentration of carbon monoxide?


A) 0.091 M
B) 0.191 M
C) 0.209 M
D) 0.913 M
E) 1.05 M

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What is the mass-action expression,Qc,for the following chemical reaction? Cu2+(aq) + 4NH3(aq) What is the mass-action expression,Q<sub>c</sub>,for the following chemical reaction? Cu<sup>2+</sup>(aq) + 4NH<sub>3</sub>(aq) Cu(NH<sub>3</sub>) <sub>4</sub><sup>2+</sup>(aq) A) B) C) D) E) None of these is the correct mass-action expression. Cu(NH3) 42+(aq)


A)
What is the mass-action expression,Q<sub>c</sub>,for the following chemical reaction? Cu<sup>2+</sup>(aq) + 4NH<sub>3</sub>(aq) Cu(NH<sub>3</sub>) <sub>4</sub><sup>2+</sup>(aq) A) B) C) D) E) None of these is the correct mass-action expression.
B)
What is the mass-action expression,Q<sub>c</sub>,for the following chemical reaction? Cu<sup>2+</sup>(aq) + 4NH<sub>3</sub>(aq) Cu(NH<sub>3</sub>) <sub>4</sub><sup>2+</sup>(aq) A) B) C) D) E) None of these is the correct mass-action expression.
C)
What is the mass-action expression,Q<sub>c</sub>,for the following chemical reaction? Cu<sup>2+</sup>(aq) + 4NH<sub>3</sub>(aq) Cu(NH<sub>3</sub>) <sub>4</sub><sup>2+</sup>(aq) A) B) C) D) E) None of these is the correct mass-action expression.
D)
What is the mass-action expression,Q<sub>c</sub>,for the following chemical reaction? Cu<sup>2+</sup>(aq) + 4NH<sub>3</sub>(aq) Cu(NH<sub>3</sub>) <sub>4</sub><sup>2+</sup>(aq) A) B) C) D) E) None of these is the correct mass-action expression.
E) None of these is the correct mass-action expression.

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