Filters
Question type
Study Flashcards

What is KP at 298 K for the following reaction? (R = 8.314 J/K • mol) SO2(g) + NO2(g) → SO3(g) + NO(g) What is K<sub>P</sub> at 298 K for the following reaction? (R = 8.314 J/K • mol) SO<sub>2</sub>(g) + NO<sub>2</sub>(g) → SO<sub>3</sub>(g) + NO(g) A) 6.99 × 10<sup>-7</sup> B) 5.71 × 10<sup>-8</sup> C) 14.2 D) 475 E) 1.42 × 10<sup>6</sup>


A) 6.99 × 10-7
B) 5.71 × 10-8
C) 14.2
D) 475
E) 1.42 × 106

Correct Answer

verifed

verified

At 500°C the equilibrium constant, KP , is 4.00 × 10-4 for the equilibrium: 2HCN(g) At 500°C the equilibrium constant, K<sub>P</sub> , is 4.00 × 10<sup>-4</sup> for the equilibrium: 2HCN(g) H<sub>2</sub>(g) + C<sub>2</sub>N<sub>2</sub>(g) What is K<sub>p</sub> for the following reaction? H<sub>2</sub>(g) + C<sub>2</sub> N<sub>2</sub>(g) 2HCN(g) A) 2.00 × 10<sup>-4</sup> B) -4.00 × 10<sup>-4</sup> C) 1.25 × 10<sup>3</sup> D) 2.50 × 10<sup>3</sup> E) 4.00 × 10<sup>4</sup> H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2 N2(g) At 500°C the equilibrium constant, K<sub>P</sub> , is 4.00 × 10<sup>-4</sup> for the equilibrium: 2HCN(g) H<sub>2</sub>(g) + C<sub>2</sub>N<sub>2</sub>(g) What is K<sub>p</sub> for the following reaction? H<sub>2</sub>(g) + C<sub>2</sub> N<sub>2</sub>(g) 2HCN(g) A) 2.00 × 10<sup>-4</sup> B) -4.00 × 10<sup>-4</sup> C) 1.25 × 10<sup>3</sup> D) 2.50 × 10<sup>3</sup> E) 4.00 × 10<sup>4</sup> 2HCN(g)


A) 2.00 × 10-4
B) -4.00 × 10-4
C) 1.25 × 103
D) 2.50 × 103
E) 4.00 × 104

Correct Answer

verifed

verified

Consider this reaction at equilibrium: 2H2O2(g) Consider this reaction at equilibrium: 2H<sub>2</sub>O<sub>2</sub>(g) 2H<sub>2</sub>O(g) + O<sub>2</sub>(g) , ΔHº<sub>rxn</sub> = -210 kJ/mol If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium? A) A shift to produce more H<sub>2</sub>O<sub>2</sub> B) A shift to produce more O<sub>2</sub> C) No change will occur. D) A shift to produce less H<sub>2</sub>O E) The pressure decreases. 2H2O(g) + O2(g) , ΔHºrxn = -210 kJ/mol If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium?


A) A shift to produce more H2O2
B) A shift to produce more O2
C) No change will occur.
D) A shift to produce less H2O
E) The pressure decreases.

Correct Answer

verifed

verified

What is the expression for the partial pressure of "A" for the following reaction under ideal conditions? A(g) What is the expression for the partial pressure of A for the following reaction under ideal conditions? A(g) B(g) A) P<sub>A</sub> = n<sub>A</sub>RT B) P<sub>A </sub>= (n<sub>A</sub>/V) RT C) P<sub>A</sub> = V/n<sub>A</sub> D) P<sub>A</sub> = VRT E) P<sub>A</sub> = (V/n<sub>A</sub>) RT B(g)


A) PA = nART
B) PA = (nA/V) RT
C) PA = V/nA
D) PA = VRT
E) PA = (V/nA) RT

Correct Answer

verifed

verified

A temperature increase favors an endothermic reaction.

Correct Answer

verifed

verified

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N2(g) + O2(g) The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N<sub>2</sub>(g) + O<sub>2</sub>(g) 2NO(g) At 2000.°C, the equilibrium constant, K<sub>c</sub>, has a value of 4.10 × 10<sup>-4</sup>. What is the value of K<sub>P</sub>? (R = 0.08206 L • atm/K • mol) A) 2.17 × 10<sup>-8</sup> B) 4.10 × 10<sup>-4</sup> C) 7.65 × 10<sup>-2</sup> D) 2.20 ×10<sup>-6</sup> E) 2.44 ×10<sup>3</sup> 2NO(g) At 2000.°C, the equilibrium constant, Kc, has a value of 4.10 × 10-4. What is the value of KP? (R = 0.08206 L • atm/K • mol)


A) 2.17 × 10-8
B) 4.10 × 10-4
C) 7.65 × 10-2
D) 2.20 ×10-6
E) 2.44 ×103

Correct Answer

verifed

verified

Sodium carbonate, Na2CO3(s) , may be prepared by heating sodium bicarbonate, NaHCO3(s) . 2NaHCO3(s) Sodium carbonate, Na<sub>2</sub>CO<sub>3</sub>(s) , may be prepared by heating sodium bicarbonate, NaHCO<sub>3</sub>(s) . 2NaHCO<sub>3</sub>(s) Na<sub>2</sub>CO<sub>3</sub>(s) + CO<sub>2</sub>(g) + H<sub>2</sub>O(g) K<sub>P</sub> = 0.23 at 100ºC If a sample of NaHCO<sub>3</sub> is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be? A) 0.46 atm B) 0.96 atm C) 0.23 atm D) 0.48 atm E) 0.11 atm Na2CO3(s) + CO2(g) + H2O(g) KP = 0.23 at 100ºC If a sample of NaHCO3 is placed in an evacuated flask and allowed to achieve equilibrium at 100ºC, what will the total gas pressure be?


A) 0.46 atm
B) 0.96 atm
C) 0.23 atm
D) 0.48 atm
E) 0.11 atm

Correct Answer

verifed

verified

For the reaction H2(g) + Br2(g) For the reaction H<sub>2</sub>(g) + Br<sub>2</sub>(g) 2HBr(g) , K<sub>c</sub> = 81.4 at 385ºC. If [H<sub>2</sub>] = [Br<sub>2</sub>] = [HBr] = 2.4 × 10<sup>-4</sup><sup>M</sup> at 385ºC, which one of the following is correct? A) [H<sub>2</sub>] and [HBr] decrease as the system moves toward equilibrium. B) The system is at equilibrium. C) [H<sub>2</sub>] and [Br<sub>2</sub>] increase as the system approaches equilibrium. D) [HBr] increases as the system approaches equilibrium. E) [HBr] and [Br<sub>2</sub>] increases as the system approaches equilibrium. 2HBr(g) , Kc = 81.4 at 385ºC. If [H2] = [Br2] = [HBr] = 2.4 × 10-4M at 385ºC, which one of the following is correct?


A) [H2] and [HBr] decrease as the system moves toward equilibrium.
B) The system is at equilibrium.
C) [H2] and [Br2] increase as the system approaches equilibrium.
D) [HBr] increases as the system approaches equilibrium.
E) [HBr] and [Br2] increases as the system approaches equilibrium.

Correct Answer

verifed

verified

The equilibrium constant for the reaction Ni(s) + 4CO(g) The equilibrium constant for the reaction Ni(s) + 4CO(g) Ni(CO) <sub>4</sub>(g) is 5.0 × 10<sup>4</sup> at 25ºC. What is the equilibrium constant for the following reaction? Ni(CO) <sub>4</sub>(g) Ni(s) + 4CO(g) ? A) 2.0 × 10<sup>-5</sup> B) 2.5 × 10<sup>9</sup> C) 5.0 × 10<sup>4</sup> D) 5.0 × 10<sup>-4</sup> E) 2.0 × 10<sup>-3</sup> Ni(CO) 4(g) is 5.0 × 104 at 25ºC. What is the equilibrium constant for the following reaction? Ni(CO) 4(g) The equilibrium constant for the reaction Ni(s) + 4CO(g) Ni(CO) <sub>4</sub>(g) is 5.0 × 10<sup>4</sup> at 25ºC. What is the equilibrium constant for the following reaction? Ni(CO) <sub>4</sub>(g) Ni(s) + 4CO(g) ? A) 2.0 × 10<sup>-5</sup> B) 2.5 × 10<sup>9</sup> C) 5.0 × 10<sup>4</sup> D) 5.0 × 10<sup>-4</sup> E) 2.0 × 10<sup>-3</sup> Ni(s) + 4CO(g) ?


A) 2.0 × 10-5
B) 2.5 × 109
C) 5.0 × 104
D) 5.0 × 10-4
E) 2.0 × 10-3

Correct Answer

verifed

verified

Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H2(g) Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H<sub>2</sub>(g) Fe(s) + H<sub>2</sub>O(g) A) K<sub>c</sub> = [H<sub>2</sub>O]/[H<sub>2</sub>] B) K<sub>c</sub> = [Fe] [H<sub>2</sub>O]/[Fe<sub>2</sub>O<sub>3</sub>] C) K<sub>c</sub> = [Fe<sub>2</sub>O<sub>3</sub>] [H<sub>2</sub>]/[Fe][H<sub>2</sub>O] D) K<sub>c</sub> = [Fe][H<sub>2</sub>O]/[Fe<sub>2</sub>O<sub>3</sub>] [H<sub>2</sub>] E) K<sub>c</sub> = [H<sub>2</sub>]/[H<sub>2</sub>O] Fe(s) + H2O(g)


A) Kc = [H2O]/[H2]
B) Kc = [Fe] [H2O]/[Fe2O3]
C) Kc = [Fe2O3] [H2]/[Fe][H2O]
D) Kc = [Fe][H2O]/[Fe2O3] [H2]
E) Kc = [H2]/[H2O]

Correct Answer

verifed

verified

A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500 K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH3OH(g) A quantity of liquid methanol, CH<sub>3</sub>OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500 K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH<sub>3</sub>OH(g) CO(g) + 2 H<sub>2</sub>(g) , K<sub>c </sub>= 6.90 × 10<sup>-2</sup> If the concentration of H<sub>2</sub> in the equilibrium mixture is 0.426 M, what mass of methanol was initially introduced into the vessel? A) 147 g B) 74.3 g C) 33.9 g D) 49.0 g E) 24.8 g CO(g) + 2 H2(g) , Kc = 6.90 × 10-2 If the concentration of H2 in the equilibrium mixture is 0.426 M, what mass of methanol was initially introduced into the vessel?


A) 147 g
B) 74.3 g
C) 33.9 g
D) 49.0 g
E) 24.8 g

Correct Answer

verifed

verified

Consider the following equilibria: 2SO3(g) Consider the following equilibria: 2SO<sub>3</sub>(g) 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) K<sub>c</sub> = 2.3 × 10<sup>-7</sup> 2NO<sub>3</sub>(g) 2NO<sub>2</sub>(g) + O<sub>2</sub>(g) K<sub>c</sub> = 1.4 × 10<sup>-3</sup> Calculate the equilibrium constant for the reaction SO<sub>2</sub>(g) + NO<sub>3</sub>(g) SO<sub>3</sub>(g) + NO<sub>2</sub>(g) . A) 78 B) 1.3 × 10<sup>-2</sup> C) 1.6 × 10<sup>-4</sup> D) 3.2 × 10<sup>-10</sup> E) 6.1 × 10<sup>3</sup> 2SO2(g) + O2(g) Kc = 2.3 × 10-7 2NO3(g) Consider the following equilibria: 2SO<sub>3</sub>(g) 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) K<sub>c</sub> = 2.3 × 10<sup>-7</sup> 2NO<sub>3</sub>(g) 2NO<sub>2</sub>(g) + O<sub>2</sub>(g) K<sub>c</sub> = 1.4 × 10<sup>-3</sup> Calculate the equilibrium constant for the reaction SO<sub>2</sub>(g) + NO<sub>3</sub>(g) SO<sub>3</sub>(g) + NO<sub>2</sub>(g) . A) 78 B) 1.3 × 10<sup>-2</sup> C) 1.6 × 10<sup>-4</sup> D) 3.2 × 10<sup>-10</sup> E) 6.1 × 10<sup>3</sup> 2NO2(g) + O2(g) Kc = 1.4 × 10-3 Calculate the equilibrium constant for the reaction SO2(g) + NO3(g) Consider the following equilibria: 2SO<sub>3</sub>(g) 2SO<sub>2</sub>(g) + O<sub>2</sub>(g) K<sub>c</sub> = 2.3 × 10<sup>-7</sup> 2NO<sub>3</sub>(g) 2NO<sub>2</sub>(g) + O<sub>2</sub>(g) K<sub>c</sub> = 1.4 × 10<sup>-3</sup> Calculate the equilibrium constant for the reaction SO<sub>2</sub>(g) + NO<sub>3</sub>(g) SO<sub>3</sub>(g) + NO<sub>2</sub>(g) . A) 78 B) 1.3 × 10<sup>-2</sup> C) 1.6 × 10<sup>-4</sup> D) 3.2 × 10<sup>-10</sup> E) 6.1 × 10<sup>3</sup> SO3(g) + NO2(g) .


A) 78
B) 1.3 × 10-2
C) 1.6 × 10-4
D) 3.2 × 10-10
E) 6.1 × 103

Correct Answer

verifed

verified

Consider the reaction: 2A(g) + B(g) → 2C(g) If ΔG° = 50.0 kJ/mol at T = 25°C and PA = PB = 1 atm and PC = 2 atm, what is the value of ΔG? (R = 8.314 J/K • mol)


A) 50.0 kJ/mol
B) 49.7 kJ/mol
C) 46.5 kJ/mol
D) 53.4 kJ/mol
E) -49.7 kJ/mol

Correct Answer

verifed

verified

Equilibrium constants are known for the following reactions: S(s) + (3/2)O2(g) Equilibrium constants are known for the following reactions: S(s) + (3/2)O<sub>2</sub>(g) SO<sub>3</sub>(g) K<sub>c</sub> = 9.2 × 10<sup>23</sup> SO<sub>3</sub>(g) SO<sub>2</sub>(g) + (1/2)O<sub>2</sub>(g) K<sub>c</sub> = 4.8 × 10<sup>-4</sup> Thus, for the reaction S(s) + O<sub>2</sub>(g) SO<sub>2</sub>(g), K<sub>c</sub> = 4.4 × 10<sup>20</sup>. SO3(g) Kc = 9.2 × 1023 SO3(g) Equilibrium constants are known for the following reactions: S(s) + (3/2)O<sub>2</sub>(g) SO<sub>3</sub>(g) K<sub>c</sub> = 9.2 × 10<sup>23</sup> SO<sub>3</sub>(g) SO<sub>2</sub>(g) + (1/2)O<sub>2</sub>(g) K<sub>c</sub> = 4.8 × 10<sup>-4</sup> Thus, for the reaction S(s) + O<sub>2</sub>(g) SO<sub>2</sub>(g), K<sub>c</sub> = 4.4 × 10<sup>20</sup>. SO2(g) + (1/2)O2(g) Kc = 4.8 × 10-4 Thus, for the reaction S(s) + O2(g) Equilibrium constants are known for the following reactions: S(s) + (3/2)O<sub>2</sub>(g) SO<sub>3</sub>(g) K<sub>c</sub> = 9.2 × 10<sup>23</sup> SO<sub>3</sub>(g) SO<sub>2</sub>(g) + (1/2)O<sub>2</sub>(g) K<sub>c</sub> = 4.8 × 10<sup>-4</sup> Thus, for the reaction S(s) + O<sub>2</sub>(g) SO<sub>2</sub>(g), K<sub>c</sub> = 4.4 × 10<sup>20</sup>. SO2(g), Kc = 4.4 × 1020.

Correct Answer

verifed

verified

The data below refer to the following reaction: 2NO(g) + I2(g) The data below refer to the following reaction: 2NO(g) + I<sub>2</sub>(g) 2NOI(g) Find the concentration of I<sub>2</sub> when the system reaches equilibrium. 2NOI(g) The data below refer to the following reaction: 2NO(g) + I<sub>2</sub>(g) 2NOI(g) Find the concentration of I<sub>2</sub> when the system reaches equilibrium. Find the concentration of I2 when the system reaches equilibrium.

Correct Answer

verifed

verified

For the reaction PCl3(g) + Cl2(g) For the reaction PCl<sub>3</sub>(g) + Cl<sub>2</sub>(g) PCl<sub>5</sub>(g) at a particular temperature, K<sub>c</sub> = 32.4. Suppose a system at that temperature is prepared with [PCl<sub>5</sub>] = 0.50 M, [Cl<sub>2</sub>] = 0.4 M, and [PCl<sub>3</sub>] = 0.10 M. Which of the following is correct? A) The system will proceed in the direction of forming more PCl<sub>5</sub> and Cl<sub>2</sub> until equilibrium is reached. B) The system is at equilibrium. C) The system will proceed in the direction of forming more PCl<sub>5</sub> until equilibrium is reached. D) The system will proceed in the direction of forming more PCl<sub>3</sub> and Cl<sub>2</sub> until equilibrium is reached. E) The system will proceed in the direction of forming more PCl<sub>3</sub> and PCl<sub>5</sub> until equilibrium is reached. PCl5(g) at a particular temperature, Kc = 32.4. Suppose a system at that temperature is prepared with [PCl5] = 0.50 M, [Cl2] = 0.4 M, and [PCl3] = 0.10 M. Which of the following is correct?


A) The system will proceed in the direction of forming more PCl5 and Cl2 until equilibrium is reached.
B) The system is at equilibrium.
C) The system will proceed in the direction of forming more PCl5 until equilibrium is reached.
D) The system will proceed in the direction of forming more PCl3 and Cl2 until equilibrium is reached.
E) The system will proceed in the direction of forming more PCl3 and PCl5 until equilibrium is reached.

Correct Answer

verifed

verified

Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4I(s) Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH<sub>4</sub>I(s) NH<sub>3</sub>(g) + HI(g) At 400°C, K<sub>P</sub> = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C. A) 0.103 atm B) 0.215 atm C) 0.232 atm D) 0.464 atm E) 2.00 atm NH3(g) + HI(g) At 400°C, KP = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.


A) 0.103 atm
B) 0.215 atm
C) 0.232 atm
D) 0.464 atm
E) 2.00 atm

Correct Answer

verifed

verified

What is the name for Qc?


A) Reversibility expression
B) Reaction expression
C) Equilibrium expression
D) Reaction quotient
E) Mass action

Correct Answer

verifed

verified

Which is the correct equilibrium constant expression for the following reaction? 2BrCl3(g) Which is the correct equilibrium constant expression for the following reaction? 2BrCl<sub>3</sub>(g) Br<sub>2</sub>(g) + 3Cl<sub>2</sub>(g) A) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]/[BrCl<sub>3</sub>] B) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]<sup>5</sup>/[BrCl<sub>3</sub>]<sup>2</sup> C) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]<sup>3</sup>/[BrCl<sub>3</sub>]<sup>2</sup> D) K<sub>c</sub> = [BrCl<sub>3</sub>]<sup>2</sup>/([Br<sub>2</sub>] × [Cl<sub>2</sub>]<sup>3</sup>) E) K<sub>c</sub> = 2[BrCl<sub>3</sub>]<sup>2</sup>/([Br<sub>2</sub>] × 3[Cl<sub>2</sub>]<sup>3</sup>) Br2(g) + 3Cl2(g)


A) Kc = [Br2] [Cl2]/[BrCl3]
B) Kc = [Br2] [Cl2]5/[BrCl3]2
C) Kc = [Br2] [Cl2]3/[BrCl3]2
D) Kc = [BrCl3]2/([Br2] × [Cl2]3)
E) Kc = 2[BrCl3]2/([Br2] × 3[Cl2]3)

Correct Answer

verifed

verified

Consider the equilibrium: A(s) Consider the equilibrium: A(s) B(s) + C(g); ΔH°<sub>rxn </sub>> 0 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 B(s) + C(g); ΔH°rxn > 0 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

Correct Answer

verifed

verified

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

View Answer

Showing 101 - 120 of 146

Related Exams

Exam 1

Chemistry: the Central Science

133 Questions

Exam 2

Atoms, Molecules, and Ions

124 Questions

Exam 3

Stoichiometry: Ratios of Combination

137 Questions

Exam 4

Reactions in Aqueous Solutions

146 Questions

Exam 5

Thermochemistry

141 Questions

Exam 6

Quantum Theory and the Electronic Structure of Atoms

135 Questions

Exam 7

Electron Configuration and the Periodic Table

120 Questions

Exam 8

Chemical Bonding I: Basic Concepts

102 Questions

Exam 9

Chemical Bonding II: Molecular Geometry and Bonding Theories

139 Questions

Exam 10

Gases

137 Questions

Exam 11

Intermolecular Forces and the Physical Properties of Liquids and Solids

137 Questions

Exam 12

Modern Materials

108 Questions

Exam 13

Physical Properties of Solutions

151 Questions

Exam 14

Chemical Kinetics

132 Questions

Exam 16

Acids and Bases

137 Questions

Exam 17

Acid-Base Equilibria and Solubility Equilibria

133 Questions

Exam 18

Entropy, Free Energy, and Equilibrium

107 Questions

Exam 19

Electrochemistry

122 Questions

Exam 20

Nuclear Chemistry

127 Questions

Exam 21

Environmental Chemistry

135 Questions

Exam 22

Coordination Chemistry

132 Questions

Exam 23

Metallurgy and the Chemistry of Metals

152 Questions

Exam 24

Nonmetallic Elements and Their Compounds

117 Questions

Exam 25

Organic Chemistry

121 Questions

Show Answer