The Kp for the reaction below is 1.49 × 108 at 100 °C: CO (g) + Cl2 (g) -COCl2 (g) In an equilibrium mixture of the three gases, PCO = PCl2 = 8.60 × 10- 4 atm. The partial pressure of the product, phosgene (COCl2), is atm.

A) 1.28 × 105 B) 1.72 × 1011 C) 1.10 × 102 D) 4.96 × 10- 15 E) 2.01 × 1014 A) 1.28 × 105 B) 1.72 × 1011 C) 1.10 × 102 D) 4.96 × 10- 15 E) 2.01 × 1014 C

At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103. 2NO (g) N2 (g) + O2 (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is Atm)

A) 294 B) 6.00 C) 18.1 D) 35.7 E) 1.50 × 10- 2 A) 294 B) 6.00 C) 18.1 D) 35.7 E) 1.50 × 10- 2 C

In the coal- gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0.35 mol of CO and 0.40 mol of H2O were placed in a 1.00- L reaction vessel. At equilibrium, there were 0.19 mol of CO remaining. Keq at the temperature of the experiment is )

A) 0.56 B) 0.75 C) 1.78 D) 5.47 E) 1.0 A) 0.56 B) 0.75 C) 1.78 D) 5.47 E) 1.0

The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g) 2NH3 (g) Is Keq = 4.34 × 10- 3 at 300 °C. At equilibrium, _ _.

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

A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is _ .

A) 4.0 B) 2.8 C) 11 D) 6.1 E) 110 A) 4.0 B) 2.8 C) 11 D) 6.1 E) 110

A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H2(g) + I2(g) When the system comes to equilibrium at 425 °C, PHI = 0.708 atm, and PH2 = PI2 = 0)0960 atm. The value of Kp at this temperature is .

A) 1.30 × 10- 2 B) 6.80 × 10- 2 C) Kp cannot be calculated for this gas reaction when the volume of the reaction vessel is not given. D) 54.3 E) 1.84 × 10- 2 A) 1.30 × 10- 2 B) 6.80 × 10- 2 C) Kp cannot be calculated for this gas reaction when the volume of the reaction vessel is not given. D) 54.3 E) 1.84 × 10- 2

At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide: H2 (g) + Br2 (g) 2HBr (g) A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.566 mol of H2 present. At equilibrium, there are Mol of Br2 present in the reaction vessel.

A) 0.440 B) 0.324 C) 0.000 D) 0.566 E) 0.232 A) 0.440 B) 0.324 C) 0.000 D) 0.566 E) 0.232

Consider the following reaction at equilibrium: 2NH3 (g) N2 (g) + 3H2 (g) OH° = +92.4 kJ Le Cha^telier's principle predicts that adding N2 (g) to the system at equilibrium will result in

A) a decrease in the concentration of NH3 (g) B) removal of all of the H2 (g) C) a lower partial pressure of N2 D) an increase in the value of the equilibrium constant E) a decrease in the concentration of H2 (g) A) a decrease in the concentration of NH3 (g) B) removal of all of the H2 (g) C) a lower partial pressure of N2 D) an increase in the value of the equilibrium constant E) a decrease in the concentration of H2 (g)

The Keq for the equilibrium below is 7.52 × 10- 2 at 480 °C.

A) 0.274 B) 3.65 C) - 0.0376 D) 13.3 E) 5.66 × 10- 3 A) 0.274 B) 3.65 C) - 0.0376 D) 13.3 E) 5.66 × 10- 3

The KS1U1B1eqS1U1B0S1U1B1 S1U1B0for the equilibrium below is 0.112 at 700 °C. SOS1U1B12 S1U1B0(g) + S1U1P1 S1S1P0S1U1P11S1S1P0S1U1P1 S1S1P0OS1U1B12S1U1B0

A) 79.7 B) 8.93 C) 17.86 D) 4.46 E) 2.99 A) 79.7 B) 8.93 C) 17.86 D) 4.46 E) 2.99

Exam 15: Chemical Equilibrium

The K_pfor the reaction below is 1.49 × 10⁸at 100 °C: CO (g) + Cl₂(g) -COCl₂(g) In an equilibrium mixture of the three gases, P_CO= P_Cl₂= 8.60 × 10^-⁴atm. The partial pressure of the product, phosgene (COCl₂), is atm.

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Question 1

Correct Answer:

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At 200 °C, the equilibrium constant (K_p) for the reaction below is 2.40 × 10³. 2NO (g) N₂(g) + O₂(g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O₂is Atm)

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Question 2

Correct Answer:

Verified

In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.

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(True/False)

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Question 3

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True

The number obtained by substituting starting reactant and product concentrations into an equilibrium- constant expression is known as the .

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Question 4

In the coal- gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H₂O (g) CO₂(g) + H₂(g) In an experiment, 0.35 mol of CO and 0.40 mol of H₂O were placed in a 1.00- L reaction vessel. At equilibrium, there were 0.19 mol of CO remaining. K_eqat the temperature of the experiment is )

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Question 5

The equilibrium constant for the gas phase reaction N₂(g) + 3H₂(g) 2NH₃(g) Is K_eq= 4.34 × 10^-³at 300 °C. At equilibrium, _ _.

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Question 6

A sealed 1.0 L flask is charged with 0.500 mol of I₂and 0.500 mol of Br₂. An equilibrium reaction ensues: I₂(g) + Br₂(g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K_eqis _ .

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Question 7

A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H₂(g) + I₂(g) ^{When the system comes to equilibrium at 425 °C, P}_HI⁼^{0.708 atm, and}^PH₂⁼^PI₂ = 0)0960 atm. The value of K_pat this temperature is .

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Question 8

At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide: H₂(g) + Br₂(g) 2HBr (g) A mixture of 0.682 mol of H₂and 0.440 mol of Br₂is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.566 mol of H₂present. At equilibrium, there are Mol of Br₂present in the reaction vessel.

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Question 9

The value of K_eqfor the equilibrium H₂(g) + I₂(g) 2 HI (g) Is 794 at 25 °C. At this temperature, what is the value of K_eqfor the equilibrium below? HI (g) 1/2 H₂(g) + 1/2 I₂(g)

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Question 10

The equilibrium- constant expression depends on the of the reaction.

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Question 11

Exactly 3.5 moles if N₂O₄is placed in an empty 2.0- L container and allowed to reach equilibrium described by the equation N₂O₄(g) "2NO₂(g) If at equilibrium the N₂O₄is 25% dissociated, what is the value of the equilibrium constant for the reaction?

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Question 12

For the endothermic reaction CaCO₃(s) CaO (s) + CO₂(g) Le Cha^{^}telier's principle predicts that _ will result in an increase in the number of moles of CO₂.

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Question 13

Consider the following reaction at equilibrium: 2NH₃(g) N₂(g) + 3H₂(g) OH° = +92.4 kJ Le Cha^{^}telier's principle predicts that adding N₂(g) to the system at equilibrium will result in

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Question 14

The K_eqfor the equilibrium below is 7.52 × 10^-²at 480 °C.

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Question 15

The effect of a catalyst on an equilibrium is to .

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Question 16

The K_eqfor the equilibrium below is 0.112 at 700 °C. SO₂(g) + ¹O₂

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Question 17

At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.

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Question 18

Le Chatelier's principle states that if a system at equilibrium is disturbed, the equilibrium will shift to minimize the disturbance.

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Question 19

In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Cha^{^}telier's principle?

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Question 20

Showing 1 - 20 of 58

Exam 15: Chemical Equilibrium

The Kp for the reaction below is 1.49 × 108 at 100 °C: CO (g) + Cl2 (g) -COCl2 (g) In an equilibrium mixture of the three gases, PCO = PCl2 = 8.60 × 10- 4 atm. The partial pressure of the product, phosgene (COCl2), is atm.

At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103. 2NO (g) N2 (g) + O2 (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is Atm)

In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.

The number obtained by substituting starting reactant and product concentrations into an equilibrium- constant expression is known as the .

The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g) 2NH3 (g) Is Keq = 4.34 × 10- 3 at 300 °C. At equilibrium, _ _.

A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is _ .

A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H2(g) + I2(g) When the system comes to equilibrium at 425 °C, PHI = 0.708 atm, and PH2 = PI2 = 0)0960 atm. The value of Kp at this temperature is .

The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) Is 794 at 25 °C. At this temperature, what is the value of Keq for the equilibrium below? HI (g) 1/2 H2 (g) + 1/2 I2 (g)

The equilibrium- constant expression depends on the of the reaction.

Exactly 3.5 moles if N2O4 is placed in an empty 2.0- L container and allowed to reach equilibrium described by the equation N2O4 (g) "2NO2 (g) If at equilibrium the N2O4 is 25% dissociated, what is the value of the equilibrium constant for the reaction?

For the endothermic reaction CaCO3 (s) CaO (s) + CO2 (g) Le Cha^telier's principle predicts that _ will result in an increase in the number of moles of CO2.

Consider the following reaction at equilibrium: 2NH3 (g) N2 (g) + 3H2 (g) OH° = +92.4 kJ Le Cha^telier's principle predicts that adding N2 (g) to the system at equilibrium will result in

The Keq for the equilibrium below is 7.52 × 10- 2 at 480 °C.

The effect of a catalyst on an equilibrium is to .

The Keq for the equilibrium below is 0.112 at 700 °C. SO2 (g) + 1 O2

At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increases the number of moles of gas in the system.

Le Chatelier's principle states that if a system at equilibrium is disturbed, the equilibrium will shift to minimize the disturbance.

In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Cha^telier's principle?

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The K_pfor the reaction below is 1.49 × 10⁸at 100 °C: CO (g) + Cl₂(g) -COCl₂(g) In an equilibrium mixture of the three gases, P_CO= P_Cl₂= 8.60 × 10^-⁴atm. The partial pressure of the product, phosgene (COCl₂), is atm.

At 200 °C, the equilibrium constant (K_p) for the reaction below is 2.40 × 10³. 2NO (g) N₂(g) + O₂(g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O₂is Atm)

The equilibrium constant for the gas phase reaction N₂(g) + 3H₂(g) 2NH₃(g) Is K_eq= 4.34 × 10^-³at 300 °C. At equilibrium, _ _.

A sealed 1.0 L flask is charged with 0.500 mol of I₂and 0.500 mol of Br₂. An equilibrium reaction ensues: I₂(g) + Br₂(g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K_eqis _ .

A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H₂(g) + I₂(g) ^{When the system comes to equilibrium at 425 °C, P}_HI⁼^{0.708 atm, and}^PH₂⁼^PI₂ = 0)0960 atm. The value of K_pat this temperature is .

The value of K_eqfor the equilibrium H₂(g) + I₂(g) 2 HI (g) Is 794 at 25 °C. At this temperature, what is the value of K_eqfor the equilibrium below? HI (g) 1/2 H₂(g) + 1/2 I₂(g)

Exactly 3.5 moles if N₂O₄is placed in an empty 2.0- L container and allowed to reach equilibrium described by the equation N₂O₄(g) "2NO₂(g) If at equilibrium the N₂O₄is 25% dissociated, what is the value of the equilibrium constant for the reaction?

For the endothermic reaction CaCO₃(s) CaO (s) + CO₂(g) Le Cha^{^}telier's principle predicts that _ will result in an increase in the number of moles of CO₂.

Consider the following reaction at equilibrium: 2NH₃(g) N₂(g) + 3H₂(g) OH° = +92.4 kJ Le Cha^{^}telier's principle predicts that adding N₂(g) to the system at equilibrium will result in

The K_eqfor the equilibrium below is 7.52 × 10^-²at 480 °C.

The K_eqfor the equilibrium below is 0.112 at 700 °C. SO₂(g) + ¹O₂

In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Cha^{^}telier's principle?