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In the gas phase, formic acid forms a dimer, 2HCOOH(g) In the gas phase, formic acid forms a dimer, 2HCOOH(g) (HCOOH) <sub>2</sub>(g) . For this reaction, ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C. Find the equilibrium constant (K<sub>P</sub>) for this reaction at 75 °C. A) 8960 B) 273 C) 0.120 D) 8.33 E) 1.12 × 10<sup>-4</sup> (HCOOH) 2(g) . For this reaction, ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C. Find the equilibrium constant (KP) for this reaction at 75 °C.


A) 8960
B) 273
C) 0.120
D) 8.33
E) 1.12 × 10-4

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

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For the endothermic reaction A2(g) For the endothermic reaction A<sub>2</sub>(g) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A<sub>2</sub>(g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the system pressure is lowered, what might the new equilibrium system look like? A) B) C) D) E) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A2(g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) For the endothermic reaction A<sub>2</sub>(g) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A<sub>2</sub>(g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the system pressure is lowered, what might the new equilibrium system look like? A) B) C) D) E) If the system pressure is lowered, what might the new equilibrium system look like?


A) For the endothermic reaction A<sub>2</sub>(g) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A<sub>2</sub>(g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the system pressure is lowered, what might the new equilibrium system look like? A) B) C) D) E)
B) For the endothermic reaction A<sub>2</sub>(g) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A<sub>2</sub>(g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the system pressure is lowered, what might the new equilibrium system look like? A) B) C) D) E)
C) For the endothermic reaction A<sub>2</sub>(g) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A<sub>2</sub>(g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the system pressure is lowered, what might the new equilibrium system look like? A) B) C) D) E)
D) For the endothermic reaction A<sub>2</sub>(g) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A<sub>2</sub>(g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the system pressure is lowered, what might the new equilibrium system look like? A) B) C) D) E)
E) For the endothermic reaction A<sub>2</sub>(g) 2A(g) , a snapshot of an equilibrium mixture of A(g) and A<sub>2</sub>(g) at low temperature may look as follows. (Each circle represents 1.0 mol of A atoms, and the volume of the box is 1.0 L.) If the system pressure is lowered, what might the new equilibrium system look like? A) B) C) D) E)

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

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At 250ºC, the equilibrium constant, KP, for the reaction PCl5(g) At 250ºC, the equilibrium constant, K<sub>P</sub>, for the reaction PCl<sub>5</sub>(g) PCl<sub>3</sub>(g) + Cl<sub>2</sub>(g) is 1.80. Sufficient PCl<sub>5</sub> is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. What is the partial pressure of PCl<sub>5</sub> after the system has reached equilibrium. A) 1.50 atm B) 1.24 atm C) 4.24 atm D) 0.94 atm E) 1.12 atm PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. What is the partial pressure of PCl5 after the system has reached equilibrium.


A) 1.50 atm
B) 1.24 atm
C) 4.24 atm
D) 0.94 atm
E) 1.12 atm

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

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The equilibrium constant, KP, for the reaction H2(g) + I2(g) The equilibrium constant, K<sub>P</sub>, for the reaction H<sub>2</sub>(g) + I<sub>2</sub>(g) 2HI(g) is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium? A) Yes. B) No, the forward reaction must proceed to establish equilibrium. C) No, the reverse reaction must proceed to establish equilibrium. D) I need to know the volume of the container before deciding. E) Need to know the starting pressures of all substances before deciding. 2HI(g) is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?


A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) I need to know the volume of the container before deciding.
E) Need to know the starting pressures of all substances before deciding.

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

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If the system 3H2(g) + N2(g) If the system 3H<sub>2</sub>(g) + N<sub>2</sub>(g) 2NH<sub>3</sub>(g) is at equilibrium and more N<sub>2</sub> is added, a net reaction that consumes some of the added N<sub>2</sub> will occur until a new equilibrium is reached. 2NH3(g) is at equilibrium and more N2 is added, a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached.

A) True
B) False

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For the following reaction at equilibrium, which one of the changes below would cause the equilibrium to shift to the left? 2NOBr(g) For the following reaction at equilibrium, which one of the changes below would cause the equilibrium to shift to the left? 2NOBr(g) 2NO(g) + Br<sub>2</sub>(g) , ΔHº<sub>rxn </sub>= 30 kJ/mol A) Increase the container volume B) Remove some NO C) Remove some Br<sub>2</sub> D) Add more NOBr E) Decrease the temperature 2NO(g) + Br2(g) , ΔHºrxn = 30 kJ/mol


A) Increase the container volume
B) Remove some NO
C) Remove some Br2
D) Add more NOBr
E) Decrease the temperature

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

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Which is correct?


A) If ΔG < 0, then Q > K.
B) If ΔG < 0, then Q < K.
C) If ΔG < 0, then Q = K.
D) If ΔGo < 0, then Q = K.
E) If ΔGo < 0, then Q > K.

F) None of the above
G) A) and D)

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Which statement is correct?


A) If Q < K, then products must be converted to reactants.
B) If Q > K, then reactants must be converted to products.
C) If Q = K, then the system is at equilibrium.
D) If Q < K, then more reactants are produced.
E) None of the answers is correct.

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

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For the reaction SO2(g) + NO2(g) For the reaction SO<sub>2</sub>(g) + NO<sub>2</sub>(g) SO<sub>3</sub>(g) + NO(g) , the equilibrium constant K<sub>c</sub> is 18.0 at 1200ºC. If 1.0 mole of SO<sub>2</sub> and 2.0 moles of NO<sub>2</sub> are placed in a 20.0-L container, what concentration of SO<sub>3</sub> will be present at equilibrium? A) 0.048 mol/L B) 0.11 mol/L C) 0.95 mol/L D) 2.22 mol/L E) 18 mol/L SO3(g) + NO(g) , the equilibrium constant Kc is 18.0 at 1200ºC. If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20.0-L container, what concentration of SO3 will be present at equilibrium?


A) 0.048 mol/L
B) 0.11 mol/L
C) 0.95 mol/L
D) 2.22 mol/L
E) 18 mol/L

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

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For ________-________ reactions KP = Kc(RT)Δn gas.

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When the concentrations of both the reactants and products remain constant because the forward and reverse reactions are occurring at the same rate then the system is ________.

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Suppose 4.2 mol of oxygen and 4.0 mol of NO are introduced to an evacuated 0.50-L reaction vessel. At a specific temperature, the equilibrium 2NO(g) + O2(g) Suppose 4.2 mol of oxygen and 4.0 mol of NO are introduced to an evacuated 0.50-L reaction vessel. At a specific temperature, the equilibrium 2NO(g) + O<sub>2</sub>(g) 2NO<sub>2</sub>(g) is reached when [NO] = 1.6 M. Calculate K<sub>c</sub> for the reaction at this temperature. 2NO2(g) is reached when [NO] = 1.6 M. Calculate Kc for the reaction at this temperature.

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The equilibrium constant, Kc, for the reaction PCl3(g) + Cl2(g) The equilibrium constant, K<sub>c</sub>, for the reaction PCl<sub>3</sub>(g) + Cl<sub>2</sub>(g) PCl<sub>5</sub>(g) is 49 at 230°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°C, what is the concentration of PCl<sub>3</sub> when equilibrium has been established? A) 0.049 M B) 0.11 M C) 0.35 M D) 0.59 M E) 0.83 M PCl5(g) is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established?


A) 0.049 M
B) 0.11 M
C) 0.35 M
D) 0.59 M
E) 0.83 M

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

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Which equation is correct?


A) ΔG = ΔG° - RT logKeq
B) ΔG° = - RT lnK
C) ΔG = RT lnQ
D) ΔG = -RT logQ
E) ΔG° = -RT logKeq

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

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The equilibrium constants (expressed in atm) for the chemical reaction N2(g) + O2(g) The equilibrium constants (expressed in atm) for the chemical reaction N<sub>2</sub>(g) + O<sub>2</sub>(g) 2NO(g) are K<sub>P</sub> = 1.1 × 10<sup>-3</sup> and 3.6 × 10<sup>-3</sup> at 2200 K and 2500 K, respectively. Which statement is true? A) The reaction is exothermic, ΔHº < 0. B) The partial pressure of NO(g) is less at 2200 K than at 2500 K. C) K<sub>p</sub> is less than K<sub>c</sub> by a factor of (RT) . D) The total pressure at 2200 K is the same as at 2500 K. E) Higher total pressure shifts the equilibrium to the left. 2NO(g) are KP = 1.1 × 10-3 and 3.6 × 10-3 at 2200 K and 2500 K, respectively. Which statement is true?


A) The reaction is exothermic, ΔHº < 0.
B) The partial pressure of NO(g) is less at 2200 K than at 2500 K.
C) Kp is less than Kc by a factor of (RT) .
D) The total pressure at 2200 K is the same as at 2500 K.
E) Higher total pressure shifts the equilibrium to the left.

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

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When a reaction system reaches equilibrium, the forward and reverse reactions stop.

A) True
B) False

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For the following reaction at 25ºC, is 3 × 1024. 2SO2(g) + O2(g) For the following reaction at 25ºC, is 3 × 10<sup>24</sup>. 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) 2SO<sub>3</sub>(g) What is K<sub>c</sub> at this temperature? (R = 0.08206 L • atm/K • mol) A) 1 × 10<sup>23</sup> B) 1 × 10<sup>24</sup> C) 3 × 10<sup>24</sup> D) 6 × 10<sup>24</sup> E) 7 × 10<sup>25</sup> 2SO3(g) What is Kc at this temperature? (R = 0.08206 L • atm/K • mol)


A) 1 × 1023
B) 1 × 1024
C) 3 × 1024
D) 6 × 1024
E) 7 × 1025

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

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For the reaction HCONH2(g) For the reaction HCONH<sub>2</sub>(g) NH<sub>3</sub>(g) + CO(g) , K<sub>c</sub> = 4.84 at 400 K. If ΔH° for this reaction is 29 kJ/mol, find K<sub>c</sub> at 500 K. A) 5.8 B) 0.17 C) 27.5 D) 0.88 E) 10.3 NH3(g) + CO(g) , Kc = 4.84 at 400 K. If ΔH° for this reaction is 29 kJ/mol, find Kc at 500 K.


A) 5.8
B) 0.17
C) 27.5
D) 0.88
E) 10.3

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

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Which is the correct mass-action expression, Qc, for the following chemical reaction? Sn2+(aq) + ½ O2(g) + 3H2O(l) Which is the correct mass-action expression, Q<sub>c</sub>, for the following chemical reaction? Sn<sup>2+</sup>(aq) + ½ O<sub>2</sub>(g) + 3H<sub>2</sub>O(l) SnO<sub>2</sub>(s) + 2H<sub>3</sub>O<sup>+</sup>(aq) A) B) C) D) E) None of these expressions is correct. SnO2(s) + 2H3O+(aq)


A) Which is the correct mass-action expression, Q<sub>c</sub>, for the following chemical reaction? Sn<sup>2+</sup>(aq) + ½ O<sub>2</sub>(g) + 3H<sub>2</sub>O(l) SnO<sub>2</sub>(s) + 2H<sub>3</sub>O<sup>+</sup>(aq) A) B) C) D) E) None of these expressions is correct.
B) Which is the correct mass-action expression, Q<sub>c</sub>, for the following chemical reaction? Sn<sup>2+</sup>(aq) + ½ O<sub>2</sub>(g) + 3H<sub>2</sub>O(l) SnO<sub>2</sub>(s) + 2H<sub>3</sub>O<sup>+</sup>(aq) A) B) C) D) E) None of these expressions is correct.
C) Which is the correct mass-action expression, Q<sub>c</sub>, for the following chemical reaction? Sn<sup>2+</sup>(aq) + ½ O<sub>2</sub>(g) + 3H<sub>2</sub>O(l) SnO<sub>2</sub>(s) + 2H<sub>3</sub>O<sup>+</sup>(aq) A) B) C) D) E) None of these expressions is correct.
D) Which is the correct mass-action expression, Q<sub>c</sub>, for the following chemical reaction? Sn<sup>2+</sup>(aq) + ½ O<sub>2</sub>(g) + 3H<sub>2</sub>O(l) SnO<sub>2</sub>(s) + 2H<sub>3</sub>O<sup>+</sup>(aq) A) B) C) D) E) None of these expressions is correct.
E) None of these expressions is correct.

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

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For any reaction, if ΔG° > 0, then K < 1.

A) True
B) False

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