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The reaction system The reaction system 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. 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.

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

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Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: The equilibrium constant for this reaction at 28 \degree C is 2900. Estimate the equilibrium constant at 38 \degree C. A) 4.7 * 10<sup>5</sup> B) 2.6 * 10<sup>4</sup> C) 1.9 * 10<sup>3</sup> D) 3.2 * 10<sup>2</sup> E) 18 The equilibrium constant for this reaction at 28 °\degree C is 2900. Estimate the equilibrium constant at 38 °\degree C.


A) 4.7 * 105
B) 2.6 * 104
C) 1.9 * 103
D) 3.2 * 102
E) 18

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

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Hydrogen iodide, HI, is formed in an equilibrium reaction when gaseous hydrogen and iodine gas are heated together. If 20.0 g of hydrogen and 20.0 g of iodine are heated, forming 10.0 g of hydrogen iodide, what mass of hydrogen remains unreacted?


A) 10.0 g hydrogen remains
B) 10.9 g hydrogen remains
C) 15.0 g hydrogen remains
D) 19.9 g hydrogen remains
E) Need to know the equilibrium constant in order to calculate the answer.

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

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What is the mass-action expression, Qp, for the following reaction? What is the mass-action expression, Q<sub>p</sub>, for the following reaction? A) B) C) D) E) None of these choices is the correct mass-action expression.


A) What is the mass-action expression, Q<sub>p</sub>, for the following reaction? A) B) C) D) E) None of these choices is the correct mass-action expression.
B) What is the mass-action expression, Q<sub>p</sub>, for the following reaction? A) B) C) D) E) None of these choices is the correct mass-action expression.
C) What is the mass-action expression, Q<sub>p</sub>, for the following reaction? A) B) C) D) E) None of these choices is the correct mass-action expression.
D) What is the mass-action expression, Q<sub>p</sub>, for the following reaction? A) B) C) D) E) None of these choices is the correct mass-action expression.
E) None of these choices is the correct mass-action expression.

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

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

A) True
B) False

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At 450 °\degree C, tert-butyl alcohol decomposes into water and isobutene. At 450 \degree C, tert-butyl alcohol decomposes into water and isobutene. A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature? A) The forward reaction will proceed to reestablish equilibrium. B) The reverse reaction will proceed to reestablish equilibrium. C) No change occurs. D) The equilibrium constant will increase. E) The equilibrium constant will decrease. A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?


A) The forward reaction will proceed to reestablish equilibrium.
B) The reverse reaction will proceed to reestablish equilibrium.
C) No change occurs.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.

F) B) and C)
G) All of the above

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A good catalyst for a reaction will speed up the forward reaction and slow down the reverse reaction.

A) True
B) False

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At 850 °\degree C, the equilibrium constant Kp for the reaction C(s) + CO2(g) At 850 \degree C, the equilibrium constant K<sub>p</sub> for the reaction C(s) + CO<sub>2</sub>(g) 2CO(g) has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide? A) 0.362 atm B) 0.489 atm C) 0.667 atm D) 0.915 atm E) 0.921 atm 2CO(g) has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?


A) 0.362 atm
B) 0.489 atm
C) 0.667 atm
D) 0.915 atm
E) 0.921 atm

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

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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 definitely 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 choices is correct.

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

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The reaction system The reaction system 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. 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.

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

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The equilibrium constant Kc for the reaction A(g) + B(g) The equilibrium constant K<sub>c</sub> for the reaction A(g) + B(g) C(g) is 0.76 at 150 \degree C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150 \degree C, what will be the equilibrium concentration of C? A) 0.19 M B) 0.29 M C) 0.36 M D) 0.41 M E) 0.51 M C(g) is 0.76 at 150 °\degree C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150 °\degree C, what will be the equilibrium concentration of C?


A) 0.19 M
B) 0.29 M
C) 0.36 M
D) 0.41 M
E) 0.51 M

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

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Ammonia is synthesized in the Haber process: Ammonia is synthesized in the Haber process:

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Kp for this reaction ...

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Consider the following two equilibria and their respective equilibrium constants: Consider the following two equilibria and their respective equilibrium constants: Which one of the following is the correct relationship between the equilibrium constants K<sub>1</sub> and K<sub>2</sub>? A) K<sub>2</sub> = 2/K<sub>1</sub> B) K<sub>2</sub> = (1/K<sub>1</sub>) <sup>2</sup> C) K<sub>2</sub> = -K<sub>1</sub>/2 D) K<sub>2</sub> = 1/(2K<sub>1</sub>) E) K<sub>2</sub> = 1/(2K<sub>1</sub>) <sup>2</sup> Which one of the following is the correct relationship between the equilibrium constants K1 and K2?


A) K2 = 2/K1
B) K2 = (1/K1) 2
C) K2 = -K1/2
D) K2 = 1/(2K1)
E) K2 = 1/(2K1) 2

F) All of the above
G) A) and B)

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Select the mass-action expression, Qc, for the following chemical reaction equation. Select the mass-action expression, Q<sub>c</sub>, for the following chemical reaction equation. A) B) C) D) E)


A) Select the mass-action expression, Q<sub>c</sub>, for the following chemical reaction equation. A) B) C) D) E)
B) Select the mass-action expression, Q<sub>c</sub>, for the following chemical reaction equation. A) B) C) D) E)
C) Select the mass-action expression, Q<sub>c</sub>, for the following chemical reaction equation. A) B) C) D) E)
D) Select the mass-action expression, Q<sub>c</sub>, for the following chemical reaction equation. A) B) C) D) E)
E) Select the mass-action expression, Q<sub>c</sub>, for the following chemical reaction equation. A) B) C) D) E)

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

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The equilibrium constant Kc for the reaction The equilibrium constant K<sub>c</sub> for the reaction is 49 at 230 \degree C. If 0.70 mol of PCl<sub>3</sub> is added to 0.70 mol of Cl<sub>2</sub> in a 1.00-L reaction vessel at 230 \degree C, what is the concentration of PCl<sub>3</sub> when equilibrium has been established? A) 0.049 M B) 0.11 M C) 0.30 M D) 0.59 M E) 0.83 M is 49 at 230 °\degree C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230 °\degree C, what is the concentration of PCl3 when equilibrium has been established?


A) 0.049 M
B) 0.11 M
C) 0.30 M
D) 0.59 M
E) 0.83 M

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

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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 choices is correct.

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

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Write the mass-action expression, Qc, for the following chemical reaction. Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)


A) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
B) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
C) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
D) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)
E) Write the mass-action expression, Q<sub>c</sub>, for the following chemical reaction. A) B) C) D) E)

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

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A chemical reaction has an equilibrium constant of 2 *106. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.


A) The forward and back reactions have stopped.
B) The limiting reactant has been used up.
C) The forward and reverse rate constants are equal.
D) The forward and reverse reaction rates are equal.
E) None of these choices is correct.

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

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What is the mass-action expression, Qc, for the following chemical reaction? What is the mass-action expression, Q<sub>c</sub>, for the following chemical reaction? A) B) C) D) E) None of these choices is correct.


A) What is the mass-action expression, Q<sub>c</sub>, for the following chemical reaction? A) B) C) D) E) None of these choices is correct.
B) What is the mass-action expression, Q<sub>c</sub>, for the following chemical reaction? A) B) C) D) E) None of these choices is correct.
C) What is the mass-action expression, Q<sub>c</sub>, for the following chemical reaction? A) B) C) D) E) None of these choices is correct.
D) What is the mass-action expression, Q<sub>c</sub>, for the following chemical reaction? A) B) C) D) E) None of these choices is correct.
E) None of these choices is correct.

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

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Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO = 0.526 atm, Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P<sub>NO</sub> = 0.526 atm, = 1.59 atm, and P<sub>NOBr</sub> = 7.68 atm. Calculate K<sub>p</sub> for the reaction. A) 7.45 * 10¯<sup>3</sup> B) 0.109 C) 9.18 D) 91.8 E) 134 = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction. Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached P<sub>NO</sub> = 0.526 atm, = 1.59 atm, and P<sub>NOBr</sub> = 7.68 atm. Calculate K<sub>p</sub> for the reaction. A) 7.45 * 10¯<sup>3</sup> B) 0.109 C) 9.18 D) 91.8 E) 134


A) 7.45 * 10¯3
B) 0.109
C) 9.18
D) 91.8
E) 134

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

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