3.2NO2 2NO + O2 Kp = 5.9 * 10 -5

A) 2 < 1 < 3 B) 1 < 2 < 3 C) 2 < 3 < 1 D) 3 < 2 < 1 E) 3 < 1 < 2 A) 2 < 1 < 3 B) 1 < 2 < 3 C) 2 < 3 < 1 D) 3 < 2 < 1 E) 3 < 1 < 2

For the reaction H2(g)+ I2(g) 2HI(g), Kc = 50.2 at 445ºC.If [H2] = [I2] = [HI] = 1.75 * 10-3 M at 445ºC, which one of these statements is true?

A) The system is at equilibrium, thus no concentration changes will occur. B) The concentrations of HI and I2 will increase as the system approaches equilibrium. C) The concentration of HI will increase as the system approaches equilibrium. D) The concentrations of H2 and HI will fall as the system moves toward equilibrium. E) The concentrations of H2 and I2 will increase as the system approaches equilibrium. A) The system is at equilibrium, thus no concentration changes will occur. B) The concentrations of HI and I2 will increase as the system approaches equilibrium. C) The concentration of HI will increase as the system approaches equilibrium. D) The concentrations of H2 and HI will fall as the system moves toward equilibrium. E) The concentrations of H2 and I2 will increase as the system approaches equilibrium.

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to decrease? 2NOBr(g) 2NO(g)+ Br2(g), $\Delta$Hºrxn= 30 kJ/mol

A) Increase the temperature. B) Remove some NO. C) Add more NOBr. D) Compress the gas mixture into a smaller volume. A) Increase the temperature. B) Remove some NO. C) Add more NOBr. D) Compress the gas mixture into a smaller volume.

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)4(g)is 5.0 * 104 at 25ºC. What is the equilibrium constant for the reaction Ni(CO)4(g) 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 A) 2.0 * 10-5 B) 2.5 * 109 C) 5.0 * 104 D) 5.0 * 10-4 E) 2.0 * 10-3

Exam 14: Chemical Equilibrium

The reaction 2NO(g) $The reaction 2NO(g) N2(g)+ O2(g)is exothermic, \Delta Hºrxn = -180 kJ/mol.Which one of these statements is true?$ N₂(g)+ O₂(g)is exothermic, $\Delta$ Hº_rxn = -180 kJ/mol.Which one of these statements is true?

(Multiple Choice)

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Question 61

3.2NO₂ 2NO + O₂ K_p = 5.9 * 10^-5

(Multiple Choice)

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Question 62

Consider this reaction at equilibrium at a total pressure P₁: 2SO₂(g)+ O₂(g) 2SO₃(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

(Multiple Choice)

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Question 63

At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g)+ Cl₂(g)is K_c = 1.6 * 10^-5. An equilibrium mixture was found to have the following concentrations of Cl₂ and NOCl: [Cl₂] = 1.2 * 10^-2M; [NOCl] = 2.8 * 10^-1M. Calculate the concentration of NO(g)at equilibrium.

(Multiple Choice)

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Question 64

When the reaction 2O₃(g) 3O₂(g), for which K_p = 3.0 * 10²⁶ at 773ºC, is at equilibrium, the mixture will contain very little O₂ as compared to O₃.

(True/False)

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Question 65

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g). The production of ammonia is an endothermic reaction.Will heating the equilibrium system increase or decrease the amount of ammonia produced?

(Essay)

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Question 66

Consider the reaction N₂(g)+ O₂(g) 2NO(g), for which K_c = 0.10 at 2,000ºC.Starting with initial concentrations of 0.040 M of N₂ and 0.040 M of O₂, determine the equilibrium concentration of NO.

(Multiple Choice)

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Question 67

What is the correct equilibrium constant expression for this reaction? 2HI(g) H₂(g)+ I₂(g)

(Essay)

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Question 68

Consider the chemical reaction 2NH₃(g) N₂(g)+ 3H₂(g).The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g)are present.Calculate K_p for the reaction.

(Short Answer)

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Question 69

For the reaction H₂(g)+ I₂(g) 2HI(g), K_c = 50.2 at 445ºC.If [H₂] = [I₂] = [HI] = 1.75 * 10^-3 M at 445ºC, which one of these statements is true?

(Multiple Choice)

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Question 70

Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide. CaCO₃(s) CaO(s)+ CO₂(g) K_P for this reaction is 1.16 at 800°C.A 5.00 L vessel containing 10.0 g of CaCO₃(s)was evacuated to remove the air, sealed, and then heated to 800°C.Ignoring the volume occupied by the solid, what will be the mass of the solid in the vessel once equilibrium is reached?

(Short Answer)

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Question 71

Two moles of PCl₅ are placed in a 5.0 L container.Dissociation takes place according to the equation PCl₅(g) PCl₃(g)+ Cl₂(g).At equilibrium, 0.40 mol of Cl₂ are present.Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

(Short Answer)

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Question 72

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g). If nitrogen is removed from the system at equilibrium, what will happen to the hydrogen (H₂)concentration?

(Short Answer)

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Question 73

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g).Which way will the reaction shift if the pressure on the system is increased?

(Short Answer)

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Question 74

In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture?

(Multiple Choice)

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Question 75

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations the products would increase, decrease, or remain constant after ammonia was added to the system.

(Short Answer)

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Question 76

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br₂ concentration to decrease? 2NOBr(g) $For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to decrease? 2NOBr(g) 2NO(g)+ Br2(g), \Delta Hºrxn= 30 kJ/mol$ 2NO(g)+ Br₂(g), $\Delta$ Hº_rxn= 30 kJ/mol

(Multiple Choice)

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Question 77

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)₄(g)is 5.0 * 10⁴ at 25ºC. What is the equilibrium constant for the reaction Ni(CO)₄(g) Ni(s)+ 4CO(g)?

(Multiple Choice)

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Question 78

Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide. CaCO₃(s) CaO(s)+ CO₂(g) K_P for this reaction is 1.16 at 800°C.A 5.00 L vessel containing 10.0 g of CaCO₃(s)was evacuated to remove the air, sealed, and then heated to 800°C.Ignoring the volume occupied by the solid, what will be the overall mass percent of carbon in the solid once equilibrium is reached?

(Short Answer)

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Question 79

The equilibrium constant expression for the reaction CuO(s)+ H₂(g) Cu(s)+ H₂O(g)is K_c = [H₂]/[H₂O].

(True/False)

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Question 80

Showing 61 - 80 of 100

Exam 14: Chemical Equilibrium

The reaction 2NO(g) N2(g)+ O2(g)is exothermic, Δ\DeltaΔ Hºrxn = -180 kJ/mol.Which one of these statements is true?

3.2NO2 2NO + O2 Kp = 5.9 * 10 -5

Consider this reaction at equilibrium at a total pressure P1: 2SO2(g)+ O2(g) 2SO3(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g)+ Cl2(g)is Kc = 1.6 * 10-5. An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 * 10-2 M; [NOCl] = 2.8 * 10-1 M. Calculate the concentration of NO(g)at equilibrium.

When the reaction 2O3(g) 3O2(g), for which Kp = 3.0 * 1026 at 773ºC, is at equilibrium, the mixture will contain very little O2 as compared to O3.

Consider the reaction N2(g)+ 3H2(g) 2NH3(g). The production of ammonia is an endothermic reaction.Will heating the equilibrium system increase or decrease the amount of ammonia produced?

Consider the reaction N2(g)+ O2(g) 2NO(g), for which Kc = 0.10 at 2,000ºC.Starting with initial concentrations of 0.040 M of N2 and 0.040 M of O2, determine the equilibrium concentration of NO.

What is the correct equilibrium constant expression for this reaction? 2HI(g) H2(g)+ I2(g)

Consider the chemical reaction 2NH3(g) N2(g)+ 3H2(g).The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 * 10-2. Initially, 1,220 moles of NH3(g)are present.Calculate Kp for the reaction.

For the reaction H2(g)+ I2(g) 2HI(g), Kc = 50.2 at 445ºC.If [H2] = [I2] = [HI] = 1.75 * 10-3 M at 445ºC, which one of these statements is true?

Two moles of PCl5 are placed in a 5.0 L container.Dissociation takes place according to the equation PCl5(g) PCl3(g)+ Cl2(g).At equilibrium, 0.40 mol of Cl2 are present.Calculate the equilibrium constant (Kc)for this reaction under the conditions of this experiment.

Consider the reaction N2(g)+ 3H2(g) 2NH3(g). If nitrogen is removed from the system at equilibrium, what will happen to the hydrogen (H2)concentration?

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J CO(g)+ H2(g).Which way will the reaction shift if the pressure on the system is increased?

In which of these gas-phase equilibria is the yield of products increased by increasing the total pressure on the reaction mixture?

Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations the products would increase, decrease, or remain constant after ammonia was added to the system.

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to decrease? 2NOBr(g) 2NO(g)+ Br2(g), Δ\DeltaΔ Hºrxn= 30 kJ/mol

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)4(g)is 5.0 * 104 at 25ºC. What is the equilibrium constant for the reaction Ni(CO)4(g) Ni(s)+ 4CO(g)?

The equilibrium constant expression for the reaction CuO(s)+ H2(g) Cu(s)+ H2O(g)is Kc = [H2]/[H2O].

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The reaction 2NO(g) $The reaction 2NO(g) <sub> </sub> N<sub>2</sub>(g)+ O<sub>2</sub>(g)is exothermic, \Delta Hº<sub>rxn</sub> = -180 kJ/mol.Which one of these statements is true?$ N₂(g)+ O₂(g)is exothermic, $\Delta$ Hº_rxn = -180 kJ/mol.Which one of these statements is true?

3.2NO₂ 2NO + O₂ K_p = 5.9 * 10^-5

Consider this reaction at equilibrium at a total pressure P₁: 2SO₂(g)+ O₂(g) 2SO₃(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g)+ Cl₂(g)is K_c = 1.6 * 10^-5. An equilibrium mixture was found to have the following concentrations of Cl₂ and NOCl: [Cl₂] = 1.2 * 10^-2M; [NOCl] = 2.8 * 10^-1M. Calculate the concentration of NO(g)at equilibrium.

When the reaction 2O₃(g) 3O₂(g), for which K_p = 3.0 * 10²⁶ at 773ºC, is at equilibrium, the mixture will contain very little O₂ as compared to O₃.

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g). The production of ammonia is an endothermic reaction.Will heating the equilibrium system increase or decrease the amount of ammonia produced?

Consider the reaction N₂(g)+ O₂(g) 2NO(g), for which K_c = 0.10 at 2,000ºC.Starting with initial concentrations of 0.040 M of N₂ and 0.040 M of O₂, determine the equilibrium concentration of NO.

What is the correct equilibrium constant expression for this reaction? 2HI(g) H₂(g)+ I₂(g)

Consider the chemical reaction 2NH₃(g) N₂(g)+ 3H₂(g).The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g)are present.Calculate K_p for the reaction.

For the reaction H₂(g)+ I₂(g) 2HI(g), K_c = 50.2 at 445ºC.If [H₂] = [I₂] = [HI] = 1.75 * 10^-3 M at 445ºC, which one of these statements is true?

Two moles of PCl₅ are placed in a 5.0 L container.Dissociation takes place according to the equation PCl₅(g) PCl₃(g)+ Cl₂(g).At equilibrium, 0.40 mol of Cl₂ are present.Calculate the equilibrium constant (K_c)for this reaction under the conditions of this experiment.

Consider the reaction N₂(g)+ 3H₂(g) 2NH₃(g). If nitrogen is removed from the system at equilibrium, what will happen to the hydrogen (H₂)concentration?

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g).Which way will the reaction shift if the pressure on the system is increased?

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations the products would increase, decrease, or remain constant after ammonia was added to the system.

The equilibrium constant for the reaction Ni(s)+ 4CO(g) Ni(CO)₄(g)is 5.0 * 10⁴ at 25ºC. What is the equilibrium constant for the reaction Ni(CO)₄(g) Ni(s)+ 4CO(g)?

The equilibrium constant expression for the reaction CuO(s)+ H₂(g) Cu(s)+ H₂O(g)is K_c = [H₂]/[H₂O].