Question 1

What is the expression for KP for the following reaction? A(g)   B(g) + 2C(g)

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 2

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr2 was 0.233 M. What is Kc for this reaction? CO(g) + Br2(g)   COBr2(g)

Accepted Answer

A)  5.23 
B)  2.14 
C)  1.17 
D)  0.467 
E)  0.191 
A)  5.23 
B)  2.14 
C)  1.17 
D)  0.467 
E)  0.191

Question 3

Nitrogen dioxide decomposes according to the reaction 2NO2(g)   2NO(g) + O2(g)
Where KP = 4.48 × 10-13 at 25°C. What is the value for Kc?(R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  1.83 × 10-14 
B)  4.48 × 10-14 
C)  9.19 × 10-13 
D)  2.18 × 10-13 
E)  1.10 × 10-11 
A)  1.83 × 10-14 
B)  4.48 × 10-14 
C)  9.19 × 10-13 
D)  2.18 × 10-13 
E)  1.10 × 10-11

Question 4

Which statement is correct?

Accepted Answer

A) If K 1, lnK is negative, and ΔG° is positive, then the reaction is product favored. C) If K > 1, lnK is positive, and ΔG° is negative, then the reaction is product favored. D) If K > 1, lnK is negative, and ΔG° is negative, then the reaction is reactant favored. E) If K < 1, lnK is positive, and ΔG° is positive, then the reaction is reactant favored. A) If K 1, lnK is negative, and ΔG° is positive, then the reaction is product favored. C) If K > 1, lnK is positive, and ΔG° is negative, then the reaction is product favored. D) If K > 1, lnK is negative, and ΔG° is negative, then the reaction is reactant favored. E) If K < 1, lnK is positive, and ΔG° is positive, then the reaction is reactant favored.

Question 5

Suppose 75.0 g of PCl5(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g), and the system is allowed to reach equilibrium at 250ºC. PCl5(g)   PCl3(g) + Cl2(g)
If Kp = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium?
(R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  6.83 atm 
B)  8.86 atm 
C)  5.38 atm 
D)  3.47 atm 
E)  1.68atm 
A)  6.83 atm 
B)  8.86 atm 
C)  5.38 atm 
D)  3.47 atm 
E)  1.68atm

Question 6

At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g)   CH3OH(g) has the value KP = 1.4 × 10-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)

Accepted Answer

A)  105 kJ/mol 
B)  1.07 kJ/mol 
C)  -233 kJ/mol 
D)  -105 kJ/mol 
E)  233 kJ/mol 
A)  105 kJ/mol 
B)  1.07 kJ/mol 
C)  -233 kJ/mol 
D)  -105 kJ/mol 
E)  233 kJ/mol

What is the expression for K_P for the following reaction? A(g) B(g) + 2C(g)

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr₂ was 0.233 M. What is K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g) + O₂(g) Where K_P = 4.48 × 10^-13 at 25°C. What is the value for K_c?(R = 0.08206 L • atm/K • mol)

Which statement is correct?

At 1500°C the equilibrium constant for the reaction CO(g) + 2H₂(g) CH₃OH(g) has the value K_P = 1.4 × 10^-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)

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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

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Electrochemistry

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Exam 15: Chemical Equilibrium

What is the expression for KP for the following reaction? A(g) B(g) + 2C(g)

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr2 was 0.233 M. What is Kc for this reaction? CO(g) + Br2(g) COBr2(g)

Nitrogen dioxide decomposes according to the reaction 2NO2(g) 2NO(g) + O2(g) Where KP = 4.48 × 10-13 at 25°C. What is the value for Kc?(R = 0.08206 L • atm/K • mol)

Which statement is correct?

Suppose 75.0 g of PCl5(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl2(g), and the system is allowed to reach equilibrium at 250ºC. PCl5(g) PCl3(g) + Cl2(g) If Kp = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium? (R = 0.08206 L • atm/K • mol)

At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) CH3OH(g) has the value KP = 1.4 × 10-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)

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

What is the expression for K_P for the following reaction? A(g) B(g) + 2C(g)

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr₂ was 0.233 M. What is K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

Nitrogen dioxide decomposes according to the reaction 2NO₂(g) 2NO(g) + O₂(g) Where K_P = 4.48 × 10^-13 at 25°C. What is the value for K_c?(R = 0.08206 L • atm/K • mol)

At 1500°C the equilibrium constant for the reaction CO(g) + 2H₂(g) CH₃OH(g) has the value K_P = 1.4 × 10^-7. What is ΔG° for this reaction at 1500°C? (R = 8.314 J/K • mol)