Hydrogen peroxide (H2O2)decomposes according to the following equation. H2O2(l)→ H2O(l)+ ½O2(g). What is KP for this reaction at 25°C? (ΔH° = -98.2 kJ/mol,ΔS° = 70.1 J/K • mol,R = 8.314 J/K• mol)

A) 1.3 × 10-21 B) 20.9 C) 3.46 × 1017 D) 7.4 × 1020 E) 8.6 × 104 A) 1.3 × 10-21 B) 20.9 C) 3.46 × 1017 D) 7.4 × 1020 E) 8.6 × 104

In the gas phase,methyl isonitrile (CH3NC)isomerizes to acetonitrile (CH3CN), H3C-N≡C(g) H3C-C≡N(g)with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C.

A) 1.68 × 10-10 B) 5.96 × 109 C) 2.16 × 1010 D) 4.63 × 10-11 E) 8.64 × 1012 A) 1.68 × 10-10 B) 5.96 × 109 C) 2.16 × 1010 D) 4.63 × 10-11 E) 8.64 × 1012

At elevated temperatures,hydrogen iodide may decompose to form hydrogen gas and iodine gas,as follows. 2HI(g) H2(g)+ I2(g) In a particular experiment,the concentrations at equilibrium were measured to be [HI] = 0.85 Mol/L,[I2] = 0.60 mol/L,and [H2] = 0.27 mol/L.What is Kc for the above reaction?

A) 5.3 B) 0.22 C) 4.5 D) 0.19 E) 1.6 × 102 A) 5.3 B) 0.22 C) 4.5 D) 0.19 E) 1.6 × 102

For the reaction H2(g)+ Br2(g) 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. 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.

At 500°C the equilibrium constant,KP ,is 4.00 ×10-4 for the equilibrium: 2HCN(g) H2(g)+ C2N2(g) What is Kp for the following reaction? H2(g)+ C2 N2(g) 2HCN(g)

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

Nitrosyl chloride (NOCl)decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g)+ Cl2(g).What is KP for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)

A) 1.60 × 10-2 B) 2.10 × 10-7 C) 62.8 D) 4.90 × 106 E) 3.20 × 109 A) 1.60 × 10-2 B) 2.10 × 10-7 C) 62.8 D) 4.90 × 106 E) 3.20 × 109

Exam 15: Chemical Equilibrium

For the reaction PCl₃(g)+ Cl₂(g) PCl₅(g)at a particular temperature,K_c = 32.4.Suppose a system at that temperature is prepared with [PCl₅] = 0.50 M,[Cl₂] = 0.4 M,and [PCl₃] = 0.10M.Which of the following is correct?

(Multiple Choice)

4.9/5

(81)

Question 41

When a reaction reaches _________,the concentration of the reactants and products will no longer change.

(Short Answer)

4.8/5

(74)

Question 42

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g)+ I₂(g),for which K_c = 0.0156 at 400ºC.Suppose 0.550 mol HI is injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of HI at equilibrium?

(Multiple Choice)

4.8/5

(79)

Question 43

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

(Multiple Choice)

4.8/5

(88)

Question 44

Hydrogen peroxide (H2O2)decomposes according to the following equation. H₂O₂(l)→ H₂O(l)+ ½O₂(g). What is K_P for this reaction at 25°C? (ΔH° = -98.2 kJ/mol,ΔS° = 70.1 J/K • mol,R = 8.314 J/K• mol)

(Multiple Choice)

4.9/5

(79)

Question 45

The reaction system POBr₃(g) POBr(g)+ Br₂(g)is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?

(Multiple Choice)

4.8/5

(90)

Question 46

What is defined as a fraction with product concentrations in the numerator and reactant concentrations in the denominator and with each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

(Multiple Choice)

4.9/5

(91)

Question 47

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position,regardless of the physical state of the substance involved.

(True/False)

4.8/5

(88)

Question 48

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g)+ I₂(g),for which K_c = 0.0156 at 400ºC.Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of H₂ at equilibrium?

(Multiple Choice)

4.8/5

(79)

Question 49

In the gas phase,methyl isonitrile (CH₃NC)isomerizes to acetonitrile (CH₃CN), H₃C-N≡C(g) H₃C-C≡N(g)with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C.

(Multiple Choice)

4.9/5

(67)

Question 50

There are guidelines to help write equilibrium constants.

(True/False)

4.8/5

(77)

Question 51

At elevated temperatures,hydrogen iodide may decompose to form hydrogen gas and iodine gas,as follows. 2HI(g) H₂(g)+ I₂(g) In a particular experiment,the concentrations at equilibrium were measured to be [HI] = 0.85 Mol/L,[I₂] = 0.60 mol/L,and [H₂] = 0.27 mol/L.What is K_c for the above reaction?

(Multiple Choice)

4.8/5

(76)

Question 52

For the reaction H₂(g)+ Br₂(g) 2HBr(g),K_c = 81.4 at 385ºC.If [H₂] = [Br₂] = [HBr] = 2.4 × 10^-4M at 385ºC,which one of the following is correct?

(Multiple Choice)

4.8/5

(82)

Question 53

When the following reaction is at equilibrium,which relationship is always true? 2NOCl(g) 2NO(g)+ Cl₂(g)

(Multiple Choice)

4.9/5

(85)

Question 54

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N₂(g)+ O₂(g) 2NO(g) The equilibrium constant K_P for the reaction is 0.0025 at 2127°C.If a container is charged with 8)00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, What will be the equilibrium partial pressure of nitrogen?

(Multiple Choice)

4.9/5

(85)

Question 55

At 500°C the equilibrium constant,K_P ,is 4.00 ×10^-4 for the equilibrium: 2HCN(g) H₂(g)+ C₂N₂(g) What is K_p for the following reaction? H₂(g)+ C₂ N₂(g) 2HCN(g)

(Multiple Choice)

4.9/5

(71)

Question 56

Nitrosyl chloride (NOCl)decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g)+ Cl₂(g).What is K_P for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)

(Multiple Choice)

4.9/5

(81)

Question 57

The following reactions occur at 500 K.Arrange them in order of increasing tendency to proceed to completion (least completion → greatest completion). 1 2NOCl 2NO + Cl₂ K_P = 1.7 × 10^{- 2} 2 N2O₄ 2NO₂ K_P = 1.5 × 10³ 3 2SO₃ 2SO₂ + O₂ K_P = 1.3 × 10^-5 4 2NO₂ 2NO + O₂ K_P = 5.9 × 10^-5

(Multiple Choice)

5.0/5

(75)

Question 58

Which equation is correct?

(Multiple Choice)

5.0/5

(77)

Question 59

For _-__ reactions K_P = K_c (RT)^Δⁿ gas.

(Short Answer)

4.9/5

(79)

Question 60

Showing 41 - 60 of 135

Exam 15: Chemical Equilibrium

For the reaction PCl3(g)+ Cl2(g) 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] = 0.10M.Which of the following is correct?

When a reaction reaches _________,the concentration of the reactants and products will no longer change.

Hydrogen iodide decomposes according to the equation 2HI(g) H2(g)+ I2(g),for which Kc = 0.0156 at 400ºC.Suppose 0.550 mol HI is injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of HI at equilibrium?

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

Hydrogen peroxide (H2O2)decomposes according to the following equation. H2O2(l)→ H2O(l)+ ½O2(g). What is KP for this reaction at 25°C? (ΔH° = -98.2 kJ/mol,ΔS° = 70.1 J/K • mol,R = 8.314 J/K• mol)

The reaction system POBr3(g) POBr(g)+ Br2(g)is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?

What is defined as a fraction with product concentrations in the numerator and reactant concentrations in the denominator and with each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?

Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position,regardless of the physical state of the substance involved.

Hydrogen iodide decomposes according to the equation 2HI(g) H2(g)+ I2(g),for which Kc = 0.0156 at 400ºC.Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of H2 at equilibrium?

In the gas phase,methyl isonitrile (CH3NC)isomerizes to acetonitrile (CH3CN), H3C-N≡C(g) H3C-C≡N(g)with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C.

There are guidelines to help write equilibrium constants.

At elevated temperatures,hydrogen iodide may decompose to form hydrogen gas and iodine gas,as follows. 2HI(g) H2(g)+ I2(g) In a particular experiment,the concentrations at equilibrium were measured to be [HI] = 0.85 Mol/L,[I2] = 0.60 mol/L,and [H2] = 0.27 mol/L.What is Kc for the above reaction?

For the reaction H2(g)+ Br2(g) 2HBr(g),Kc = 81.4 at 385ºC.If [H2] = [Br2] = [HBr] = 2.4 × 10-4M at 385ºC,which one of the following is correct?

When the following reaction is at equilibrium,which relationship is always true? 2NOCl(g) 2NO(g)+ Cl2(g)

At 500°C the equilibrium constant,KP ,is 4.00 ×10-4 for the equilibrium: 2HCN(g) H2(g)+ C2N2(g) What is Kp for the following reaction? H2(g)+ C2 N2(g) 2HCN(g)

Nitrosyl chloride (NOCl)decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g)+ Cl2(g).What is KP for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)

The following reactions occur at 500 K.Arrange them in order of increasing tendency to proceed to completion (least completion → greatest completion). 1 2NOCl 2NO + Cl2 KP = 1.7 × 10- 2 2 N2O4 2NO2 KP = 1.5 × 103 3 2SO3 2SO2 + O2 KP = 1.3 × 10 -5 4 2NO2 2NO + O2 KP = 5.9 × 10 -5

Which equation is correct?

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

Chemistry: the Central Science

Atoms Molecules and Ions

Stoichiometry Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I Basic Concepts

Chemical Bonding Ii Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

For the reaction PCl₃(g)+ Cl₂(g) PCl₅(g)at a particular temperature,K_c = 32.4.Suppose a system at that temperature is prepared with [PCl₅] = 0.50 M,[Cl₂] = 0.4 M,and [PCl₃] = 0.10M.Which of the following is correct?

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g)+ I₂(g),for which K_c = 0.0156 at 400ºC.Suppose 0.550 mol HI is injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of HI at equilibrium?

Hydrogen peroxide (H2O2)decomposes according to the following equation. H₂O₂(l)→ H₂O(l)+ ½O₂(g). What is K_P for this reaction at 25°C? (ΔH° = -98.2 kJ/mol,ΔS° = 70.1 J/K • mol,R = 8.314 J/K• mol)

The reaction system POBr₃(g) POBr(g)+ Br₂(g)is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g)+ I₂(g),for which K_c = 0.0156 at 400ºC.Suppose 0.550 mol HI was injected into a 2.00-L reaction vessel at 400ºC.What is the concentration of H₂ at equilibrium?

In the gas phase,methyl isonitrile (CH₃NC)isomerizes to acetonitrile (CH₃CN), H₃C-N≡C(g) H₃C-C≡N(g)with ΔH° = -89.5 kJ/mol and ΔG° = - 73.8 kJ/mol at 25°C.Find the equilibrium constant for this reaction at 100°C.

For the reaction H₂(g)+ Br₂(g) 2HBr(g),K_c = 81.4 at 385ºC.If [H₂] = [Br₂] = [HBr] = 2.4 × 10^-4M at 385ºC,which one of the following is correct?

When the following reaction is at equilibrium,which relationship is always true? 2NOCl(g) 2NO(g)+ Cl₂(g)

At 500°C the equilibrium constant,K_P ,is 4.00 ×10^-4 for the equilibrium: 2HCN(g) H₂(g)+ C₂N₂(g) What is K_p for the following reaction? H₂(g)+ C₂ N₂(g) 2HCN(g)

Nitrosyl chloride (NOCl)decomposes at elevated temperatures according to the equation 2NOCl(g) 2NO(g)+ Cl₂(g).What is K_P for this reaction at 227°C? For this reaction ΔH° = 81.2 kJ/mol and ΔS° = 128 J/K • mol.(R = 8.314 J/K • mol)

For _-__ reactions K_P = K_c (RT)^Δⁿ gas.