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 0.556 mol of H2 present. At equilibrium, there are __________ mol of Br2 present in the reaction vessel.

A) 0.000 B) 0.440 C) 0.556 D) 0.126 E) 0.314 A) 0.000 B) 0.440 C) 0.556 D) 0.126 E) 0.314

The Keq for the equilibrium below is 7.52 × 10-2 at 480.0°C. 2Cl2 (g)+ 2H2O (g) 4HCl (g)+ O2 (g) What is the value of Keq at this temperature for the following reaction? 4HCl (g)+ O2 (g) 2Cl2 (g)+ 2H2O (g)

A) 0.0752 B) -0.0752 C) 13.3 D) 5.66 × 10-3 E) 0.150 A) 0.0752 B) -0.0752 C) 13.3 D) 5.66 × 10-3 E) 0.150

The Keq for the equilibrium below is 7.52 × 10-2 at 480.0°C. 2Cl2 (g)+ 2H2O (g) 4HCl (g)+ O2 (g) What is the value of Keq at this temperature for the following reaction? 2HCl (g)+ O2 (g) Cl2 (g)+ H2O (g)

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

At 1000.0 K, the equilibrium constant for the reaction 2NO (g)+ Br2 (g) 2NOBr (g) Is Kp = 0.017. Calculate Kp for the reverse reaction, 2NOBr (g) 2NO (g)+ Br2 (g).

A) 0.017 B) 1.6 × 10-4 C) 59 D) 0.99 E) 1.1 A) 0.017 B) 1.6 × 10-4 C) 59 D) 0.99 E) 1.1

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

The value of Keq for the equilibrium N2 (g)+ O2 (g) 2 NO (g) Is 4.2 × 10-31 at 27 °C. What is the value of Keq for the equilibrium below? 4 NO (g) 2 N2 (g)+ 2 O2 (g)

A) 5.7 × 1060 B) 8.4 × 10-31 C) 4.2 × 1031 D) 8.4 × 1031 E) none of the above A) 5.7 × 1060 B) 8.4 × 10-31 C) 4.2 × 1031 D) 8.4 × 1031 E) none of the above

Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g)+ O2 (g)ΔH° = -514 kJ Le Châtelier's principle predicts that an increase in temperature will __________.

A) increase the partial pressure of O2 (g) B) decrease the partial pressure of CO2 (g) C) decrease the value of the equilibrium constant D) increase the value of the equilibrium constant E) increase the partial pressure of CO A) increase the partial pressure of O2 (g) B) decrease the partial pressure of CO2 (g) C) decrease the value of the equilibrium constant D) increase the value of the equilibrium constant E) increase the partial pressure of CO

The Keq for the equilibrium below is 7.73 × 10-2 at 500.0°C. 2Cl2 (g)+ 2H2O (g) 4HCl (g)+ O2 (g) What is the value of Keq at this temperature for the following reaction? Cl2 (g)+ H2O (g) 2HCl (g)+ O2 (g)

A) 0.0773 B) 5.98 × 10-3 C) 0.278 D) 0.0376 E) 0.150 A) 0.0773 B) 5.98 × 10-3 C) 0.278 D) 0.0376 E) 0.150

The Keq for the equilibrium below is 5.4 × 1013 at 480.0°C. 2NO (g)+ O2 (g) 2NO2 (g) What is the value of Keq at this temperature for the following reaction? 4NO (g)+ 2O2 (g) 4NO2 (g)

A) 5.4 × 1013 B) 5.4 × 10-13 C) 1.9 × 1012 D) 1.9 × 10-12 E) 2.9 × 1027 A) 5.4 × 1013 B) 5.4 × 10-13 C) 1.9 × 1012 D) 1.9 × 10-12 E) 2.9 × 1027

Consider the following reaction at equilibrium: C (s)+ H2O (g) CO (g)+ H2 (g) Which of the following conditions will increase the partial pressure of CO?

A) decreasing the partial pressure of H2O (g) B) removing H2O (g)from the system C) decreasing the volume of the reaction vessel D) decreasing the pressure in the reaction vessel E) increasing the amount of carbon in the system A) decreasing the partial pressure of H2O (g) B) removing H2O (g)from the system C) decreasing the volume of the reaction vessel D) decreasing the pressure in the reaction vessel E) increasing the amount of carbon in the system

The value of Keq for the following reaction is 0.25: SO2 (g)+ NO2 (g) SO3 (g)+ NO (g) The value of Keq at the same temperature for the reaction below is __________. 2SO2 (g)+ 2NO2 (g) 2SO3 (g)+ 2NO (g)

A) 0.50 B) 0.063 C) 0.12 D) 0.25 E) 16 A) 0.50 B) 0.063 C) 0.12 D) 0.25 E) 16

Given the following reaction at equilibrium at 300.0 K: NH4HS (s) NH3 (g)+ H2S (g) If pNH3 = pH2S = 0.109 atm, Kp = __________.

A) .0119 B) 4.99 × 10-4 C) .109 D) .0821 E) 5.66 × 10-3 A) .0119 B) 4.99 × 10-4 C) .109 D) .0821 E) 5.66 × 10-3

The value of Keq for the equilibrium H2 (g)+ I2 (g) 2 HI (g) Is 54.0 at 427°C. What is the value of Keq for the equilibrium below? HI (g) 1/2 H2 (g)+ 1/2 I2 (g)

A) 27 B) 7.35 C) 0.136 D) 2.92 × 103 E) 3.43 × 10-4 A) 27 B) 7.35 C) 0.136 D) 2.92 × 103 E) 3.43 × 10-4

Exam 15: Chemical Equilibrium

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 0.556 mol of H₂ present. At equilibrium, there are __________ mol of Br₂ present in the reaction vessel.

(Multiple Choice)

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Question 41

The K_eq for the equilibrium below is 7.52 × 10^-2 at 480.0°C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g) What is the value of K_eq at this temperature for the following reaction? 4HCl (g)+ O₂ (g) 2Cl₂ (g)+ 2H₂O (g)

(Multiple Choice)

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Question 42

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

(Multiple Choice)

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Question 43

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is __________. (1)SO₂ (g)+ (1/2)O₂ (g) SO₃ (g) (2)2SO₃ (g) 2SO₂ (g)+ O₂ (g)

(Multiple Choice)

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Question 44

The expression for K_p for the reaction below is __________. 4CuO (s)+ CH₄ (g) CO₂ (g)+ 4Cu (s)+ 2H₂O (g)

(Multiple Choice)

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Question 45

The K_eq for the equilibrium below is 7.52 × 10^-2 at 480.0°C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g) What is the value of K_eq at this temperature for the following reaction? 2HCl (g)+ O₂ (g) Cl₂ (g)+ H₂O (g)

(Multiple Choice)

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Question 46

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

(Multiple Choice)

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Question 47

If the reaction quotient Q for a reaction is less than the value of the equilibrium constant K for that reaction at a given temperature, must be converted to for the system to reach equilibrium.

(Short Answer)

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Question 48

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N₂O₄ (g) 2NO₂ (g)

(Multiple Choice)

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Question 49

At 1000.0 K, the equilibrium constant for the reaction 2NO (g)+ Br₂ (g) 2NOBr (g) Is K_p = 0.017. Calculate K_p for the reverse reaction, 2NOBr (g) 2NO (g)+ Br₂(g).

(Multiple Choice)

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Question 50

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_p at this temperature is __________.

(Multiple Choice)

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Question 51

The value of K_eq for the equilibrium N₂ (g)+ O₂ (g) 2 NO (g) Is 4.2 × 10^-31 at 27 °C. What is the value of K_eq for the equilibrium below? 4 NO (g) 2 N₂ (g)+ 2 O₂ (g)

(Multiple Choice)

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Question 52

Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g)+ O₂ (g)ΔH° = -514 kJ Le Châtelier's principle predicts that an increase in temperature will __________.

(Multiple Choice)

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Question 53

The K_eq for the equilibrium below is 7.73 × 10^-2 at 500.0°C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g) What is the value of K_eq at this temperature for the following reaction? Cl₂ (g)+ H₂O (g) 2HCl (g)+ O₂ (g)

(Multiple Choice)

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Question 54

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

(Multiple Choice)

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Question 55

The K_eq for the equilibrium below is 5.4 × 10¹³ at 480.0°C. 2NO (g)+ O₂ (g) 2NO₂ (g) What is the value of K_eq at this temperature for the following reaction? 4NO (g)+ 2O₂ (g) 4NO₂ (g)

(Multiple Choice)

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Question 56

Consider the following reaction at equilibrium: C (s)+ H₂O (g) CO (g)+ H₂ (g) Which of the following conditions will increase the partial pressure of CO?

(Multiple Choice)

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Question 57

The value of K_eq for the following reaction is 0.25: SO₂ (g)+ NO₂ (g) SO₃ (g)+ NO (g) The value of K_eq at the same temperature for the reaction below is __________. 2SO₂ (g)+ 2NO₂ (g) 2SO₃ (g)+ 2NO (g)

(Multiple Choice)

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Question 58

Given the following reaction at equilibrium at 300.0 K: NH₄HS (s) NH₃ (g)+ H₂S (g) If pNH₃ = pH₂S = 0.109 atm, K_p = __________.

(Multiple Choice)

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Question 59

The value of K_eq for the equilibrium H₂ (g)+ I₂ (g) 2 HI (g) Is 54.0 at 427°C. What is the value of K_eq for the equilibrium below? HI (g) 1/2 H₂ (g)+ 1/2 I₂ (g)

(Multiple Choice)

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Question 60

Showing 41 - 60 of 92

Exam 15: Chemical Equilibrium

The Keq for the equilibrium below is 7.52 × 10-2 at 480.0°C. 2Cl2 (g)+ 2H2O (g) 4HCl (g)+ O2 (g) What is the value of Keq at this temperature for the following reaction? 4HCl (g)+ O2 (g) 2Cl2 (g)+ 2H2O (g)

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

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is __________. (1)SO2 (g)+ (1/2)O2 (g) SO3 (g) (2)2SO3 (g) 2SO2 (g)+ O2 (g)

The expression for Kp for the reaction below is __________. 4CuO (s)+ CH4 (g) CO2 (g)+ 4Cu (s)+ 2H2O (g)

The Keq for the equilibrium below is 7.52 × 10-2 at 480.0°C. 2Cl2 (g)+ 2H2O (g) 4HCl (g)+ O2 (g) What is the value of Keq at this temperature for the following reaction? 2HCl (g)+ O2 (g) Cl2 (g)+ H2O (g)

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

If the reaction quotient Q for a reaction is less than the value of the equilibrium constant K for that reaction at a given temperature, __________ must be converted to __________ for the system to reach equilibrium.

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N2O4 (g) 2NO2 (g)

At 1000.0 K, the equilibrium constant for the reaction 2NO (g)+ Br2 (g) 2NOBr (g) Is Kp = 0.017. Calculate Kp for the reverse reaction, 2NOBr (g) 2NO (g)+ Br2 (g).

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 N2 (g)+ O2 (g) 2 NO (g) Is 4.2 × 10-31 at 27 °C. What is the value of Keq for the equilibrium below? 4 NO (g) 2 N2 (g)+ 2 O2 (g)

Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g)+ O2 (g)ΔH° = -514 kJ Le Châtelier's principle predicts that an increase in temperature will __________.

The Keq for the equilibrium below is 7.73 × 10-2 at 500.0°C. 2Cl2 (g)+ 2H2O (g) 4HCl (g)+ O2 (g) What is the value of Keq at this temperature for the following reaction? Cl2 (g)+ H2O (g) 2HCl (g)+ O2 (g)

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

The Keq for the equilibrium below is 5.4 × 1013 at 480.0°C. 2NO (g)+ O2 (g) 2NO2 (g) What is the value of Keq at this temperature for the following reaction? 4NO (g)+ 2O2 (g) 4NO2 (g)

Consider the following reaction at equilibrium: C (s)+ H2O (g) CO (g)+ H2 (g) Which of the following conditions will increase the partial pressure of CO?

The value of Keq for the following reaction is 0.25: SO2 (g)+ NO2 (g) SO3 (g)+ NO (g) The value of Keq at the same temperature for the reaction below is __________. 2SO2 (g)+ 2NO2 (g) 2SO3 (g)+ 2NO (g)

Given the following reaction at equilibrium at 300.0 K: NH4HS (s) NH3 (g)+ H2S (g) If pNH3 = pH2S = 0.109 atm, Kp = __________.

The value of Keq for the equilibrium H2 (g)+ I2 (g) 2 HI (g) Is 54.0 at 427°C. What is the value of Keq for the equilibrium below? HI (g) 1/2 H2 (g)+ 1/2 I2 (g)

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The K_eq for the equilibrium below is 7.52 × 10^-2 at 480.0°C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g) What is the value of K_eq at this temperature for the following reaction? 4HCl (g)+ O₂ (g) 2Cl₂ (g)+ 2H₂O (g)

The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is __________. (1)SO₂ (g)+ (1/2)O₂ (g) SO₃ (g) (2)2SO₃ (g) 2SO₂ (g)+ O₂ (g)

The expression for K_p for the reaction below is __________. 4CuO (s)+ CH₄ (g) CO₂ (g)+ 4Cu (s)+ 2H₂O (g)

The K_eq for the equilibrium below is 7.52 × 10^-2 at 480.0°C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g) What is the value of K_eq at this temperature for the following reaction? 2HCl (g)+ O₂ (g) Cl₂ (g)+ H₂O (g)

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

If the reaction quotient Q for a reaction is less than the value of the equilibrium constant K for that reaction at a given temperature, must be converted to for the system to reach equilibrium.

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N₂O₄ (g) 2NO₂ (g)

At 1000.0 K, the equilibrium constant for the reaction 2NO (g)+ Br₂ (g) 2NOBr (g) Is K_p = 0.017. Calculate K_p for the reverse reaction, 2NOBr (g) 2NO (g)+ Br₂(g).

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_p at this temperature is __________.

The value of K_eq for the equilibrium N₂ (g)+ O₂ (g) 2 NO (g) Is 4.2 × 10^-31 at 27 °C. What is the value of K_eq for the equilibrium below? 4 NO (g) 2 N₂ (g)+ 2 O₂ (g)

Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g)+ O₂ (g)ΔH° = -514 kJ Le Châtelier's principle predicts that an increase in temperature will __________.

The K_eq for the equilibrium below is 7.73 × 10^-2 at 500.0°C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g) What is the value of K_eq at this temperature for the following reaction? Cl₂ (g)+ H₂O (g) 2HCl (g)+ O₂ (g)

The K_eq for the equilibrium below is 5.4 × 10¹³ at 480.0°C. 2NO (g)+ O₂ (g) 2NO₂ (g) What is the value of K_eq at this temperature for the following reaction? 4NO (g)+ 2O₂ (g) 4NO₂ (g)

Consider the following reaction at equilibrium: C (s)+ H₂O (g) CO (g)+ H₂ (g) Which of the following conditions will increase the partial pressure of CO?

The value of K_eq for the following reaction is 0.25: SO₂ (g)+ NO₂ (g) SO₃ (g)+ NO (g) The value of K_eq at the same temperature for the reaction below is __________. 2SO₂ (g)+ 2NO₂ (g) 2SO₃ (g)+ 2NO (g)

Given the following reaction at equilibrium at 300.0 K: NH₄HS (s) NH₃ (g)+ H₂S (g) If pNH₃ = pH₂S = 0.109 atm, K_p = __________.

The value of K_eq for the equilibrium H₂ (g)+ I₂ (g) 2 HI (g) Is 54.0 at 427°C. What is the value of K_eq for the equilibrium below? HI (g) 1/2 H₂ (g)+ 1/2 I₂ (g)