Question 1

Write an expression for the equilibrium constant (Keq) for the following reaction.   (g) +   (g)   2HF (g)

Accepted Answer

The answer of Write an expression for the equilibrium constant...

Question 2

Changing the temperature of a reaction will not change the equilibrium value.

Accepted Answer

A) True 
 B)False

Question 3

Predict the shift in the direction of the reaction for the following chemical reaction:
4HCl (g) +   (g)     (g) +   O (g)
a) if water (   O) is added
b) if chlorine (   ) is removed
c) if oxygen (   ) is removed

Accepted Answer

a) shift l

Question 4

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift.
-2 C?H?? (g) + 25 O? (g)

Accepted Answer

A) no effect 
B) right (?) 
C) left (?) 
A) no effect 
B) right (?) 
C) left (?)

Question 5

Write an expression for the equilibrium constant (Keq) for the following reaction.       (aq) +   O (l)         + (aq) + OH- (aq)

Accepted Answer

Keq = [ @#IMG-DLM& @#IMG-DLM&

Question 6

If the value of the equilibrium constant for the forward reaction is 5.0 × 1010, the value of the equilibrium constant for the reverse reaction is ________.

Accepted Answer

A)  -5.0 × 1030 
B)  5.0 × 10-10 
C)  2.0 × 10-11 
D)  2.0 × 10-10 
A)  -5.0 × 1030 
B)  5.0 × 10-10 
C)  2.0 × 10-11 
D)  2.0 × 10-10

Question 7

If the value of the equilibrium constant for the forward reaction is 2.5 × 1030, the value of the equilibrium constant for the reverse reaction is 4.0 × 10-30.

Accepted Answer

A) True 
 B)False

Question 8

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift.
-O₂ (g) + 2 F₂ (g)   2 OF₂ (g)

Accepted Answer

A) left (←) 
B) right (→) 
A) left (←) 
B) right (→)

Question 9

Among the two reactions whose equilibrium constants are 0.003 and 30, the one that will produce greater quantities of products is the one whose equilibrium constant is 30.

Accepted Answer

A) True 
 B)False

Question 10

At 500 K, the equilibrium concentrations of each species are [PCl5] = 0.008 M, [PCL₃] = 0.02 M, and [CL₂] = 0.02 M. The equilibrium constant value is 0.5.
PCl5 ⇔ PCL₃ + CL₂

Accepted Answer

A) True 
 B)False

Question 11

Reducing the pressure will shift the equilibrium to the right.
CL₂ (g) + 3F₂ (g) ⇔ 2ClF3 (g)

Accepted Answer

A) True 
 B)False

Question 12

At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.

Accepted Answer

A) True 
 B)False

Question 13

Which of the following statements about the equilibrium constant is incorrect?

Accepted Answer

A) If Keq > 1 the reaction favors product formation. B) If Keq > 1 the reaction does not favor product formation. C) If Keq = 1 the reaction is at equilibrium. D) If Keq < 1 the reaction does not favor product formation. A) If Keq > 1 the reaction favors product formation. B) If Keq > 1 the reaction does not favor product formation. C) If Keq = 1 the reaction is at equilibrium. D) If Keq < 1 the reaction does not favor product formation.

Question 14

An equilibrium condition can be achieved only when 100% of the reactants have been converted to products.

Accepted Answer

A) True 
 B)False

Question 15

If   is removed from the following reaction already at equilibrium:   +     2HI
what would be expected to happen to the rate of the reverse reaction?

Accepted Answer

The rate of the reverse reacti

Write an expression for the equilibrium constant (Keq) for the following reaction. (g) + (g) 2HF (g)

Changing the temperature of a reaction will not change the equilibrium value.

Predict the shift in the direction of the reaction for the following chemical reaction: 4HCl (g) + (g) (g) + O (g) a) if water ( O) is added b) if chlorine ( ) is removed c) if oxygen ( ) is removed

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -2 C?H?? (g) + 25 O? (g)

Write an expression for the equilibrium constant (Keq) for the following reaction. (aq) + O (l) + (aq) + OH- (aq)

If the value of the equilibrium constant for the forward reaction is 5.0 × 10¹⁰, the value of the equilibrium constant for the reverse reaction is ________.

If the value of the equilibrium constant for the forward reaction is 2.5 × 10³⁰, the value of the equilibrium constant for the reverse reaction is 4.0 × 10^-30.

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -O₂ (g) + 2 F₂ (g) 2 OF₂ (g)

Among the two reactions whose equilibrium constants are 0.003 and 30, the one that will produce greater quantities of products is the one whose equilibrium constant is 30.

At 500 K, the equilibrium concentrations of each species are [PCl₅] = 0.008 M, [PCL₃] = 0.02 M, and [CL₂] = 0.02 M. The equilibrium constant value is 0.5. PCl5 ⇔ PCL₃ + CL₂

Reducing the pressure will shift the equilibrium to the right. CL₂ (g) + 3F₂ (g) ⇔ 2ClF3 (g)

At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.

Which of the following statements about the equilibrium constant is incorrect?

An equilibrium condition can be achieved only when 100% of the reactants have been converted to products.

If is removed from the following reaction already at equilibrium: + 2HI what would be expected to happen to the rate of the reverse reaction?

What Is Chemistry

The Numerical Side of Chemistry

The Evolution of Atomic Theory

The Modern Model of the Atom

Chemical Bonding and Nomenclature

The Shape of Molecules

Intermolecular Forces and the Phases of Matter

Chemical Reactions

Stoichiometry and the Mole

Electron Transfer in Chemical Reactions

What If There Were No Intermolecular Forces - the Ideal Gas

Solutions

When Reactants Turn Into Products

Electrolytes, Acids, and Bases

Nuclear Chemistry

The Chemistry of Carbon

Synthetic and Biological Polymers

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Exam 14: Chemical Equilibrium

Write an expression for the equilibrium constant (Keq) for the following reaction. (g) + (g) 2HF (g)

Changing the temperature of a reaction will not change the equilibrium value.

Predict the shift in the direction of the reaction for the following chemical reaction: 4HCl (g) + (g) (g) + O (g) a) if water ( O) is added b) if chlorine ( ) is removed c) if oxygen ( ) is removed

Predict the effect of increasing pressure in each of the reactions by choosing the appropriate direction shift. -2 C?H?? (g) + 25 O? (g)

Write an expression for the equilibrium constant (Keq) for the following reaction. (aq) + O (l) + (aq) + OH- (aq)

If the value of the equilibrium constant for the forward reaction is 5.0 × 1010, the value of the equilibrium constant for the reverse reaction is ________.

If the value of the equilibrium constant for the forward reaction is 2.5 × 1030, the value of the equilibrium constant for the reverse reaction is 4.0 × 10-30.

Predict the effect of increasing the concentration of the bolded species in each of the balanced equations by choosing the appropriate direction shift. -O₂ (g) + 2 F₂ (g) 2 OF₂ (g)

Among the two reactions whose equilibrium constants are 0.003 and 30, the one that will produce greater quantities of products is the one whose equilibrium constant is 30.

At 500 K, the equilibrium concentrations of each species are [PCl5] = 0.008 M, [PCL₃] = 0.02 M, and [CL₂] = 0.02 M. The equilibrium constant value is 0.5. PCl5 ⇔ PCL₃ + CL₂

Reducing the pressure will shift the equilibrium to the right. CL₂ (g) + 3F₂ (g) ⇔ 2ClF3 (g)

At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.

Which of the following statements about the equilibrium constant is incorrect?

An equilibrium condition can be achieved only when 100% of the reactants have been converted to products.

If is removed from the following reaction already at equilibrium: + 2HI what would be expected to happen to the rate of the reverse reaction?

What Is Chemistry

The Numerical Side of Chemistry

The Evolution of Atomic Theory

The Modern Model of the Atom

Chemical Bonding and Nomenclature

The Shape of Molecules

Intermolecular Forces and the Phases of Matter

Chemical Reactions

Stoichiometry and the Mole

Electron Transfer in Chemical Reactions

What If There Were No Intermolecular Forces - the Ideal Gas

Solutions

When Reactants Turn Into Products

Electrolytes, Acids, and Bases

Nuclear Chemistry

The Chemistry of Carbon

Synthetic and Biological Polymers

Filters

If the value of the equilibrium constant for the forward reaction is 5.0 × 10¹⁰, the value of the equilibrium constant for the reverse reaction is ________.

If the value of the equilibrium constant for the forward reaction is 2.5 × 10³⁰, the value of the equilibrium constant for the reverse reaction is 4.0 × 10^-30.

At 500 K, the equilibrium concentrations of each species are [PCl₅] = 0.008 M, [PCL₃] = 0.02 M, and [CL₂] = 0.02 M. The equilibrium constant value is 0.5. PCl5 ⇔ PCL₃ + CL₂