Question 1

What is the value for the   for a compound MX(s)if at equilibrium

Accepted Answer

A) 0.0020 
B) 1.0 ×   
C) 1.0 ×   
D) not enough information 
E) none of the above 
A) 0.0020 
B) 1.0 ×   
C) 1.0 ×   
D) not enough information 
E) none of the above

Question 2

The equilibrium expression for the reaction:   .

Accepted Answer

A) True 
 B)False

Question 3

For the reaction  
what happens to the equilibrium position if the volume increases?

Accepted Answer

A) shifts to the left 
B) shifts to the right 
C) does nothing 
D) doubles 
E) halves 
A) shifts to the left 
B) shifts to the right 
C) does nothing 
D) doubles 
E) halves

Question 4

Iron(II)carbonate (   = 3.07 × 10-11)is more soluble than calcium fluoride (   = 1.46 × 10-10).

Accepted Answer

A) True 
 B)False

Question 5

As long as Keq> 1,all reactants will eventually be consumed and leave us exclusively with product molecules.

Accepted Answer

A) True 
 B)False

Question 6

Which of the following is TRUE of a system for which   >> 1?

Accepted Answer

A) It will take a short time to reach equilibrium. 
B) It will take a long time to reach equilibrium. 
C) The equilibrium favors the reverse reaction. 
D) The equilibrium favors the forward reaction. 
E) none of the above 
A) It will take a short time to reach equilibrium. 
B) It will take a long time to reach equilibrium. 
C) The equilibrium favors the reverse reaction. 
D) The equilibrium favors the forward reaction. 
E) none of the above

Question 7

A reaction that has Keq = 2.0 × 10-8 will have high concentrations of products.

Accepted Answer

A) True 
 B)False

Question 8

A compound with a very large   value is generally considered to be only partially soluble.

Accepted Answer

A) True 
 B)False

Question 9

Decreasing the volume of the system below causes the reaction to shift towards the right.

Accepted Answer

A) True 
 B)False

Question 10

A description of life is:

Accepted Answer

A) Living things maintain and control their sameness. 
B) Living things maintain and control their changelessness. 
C) Living things maintain and control their equilibrium. 
D) Living things maintain and control their disequilibrium. 
E) none of the above 
A) Living things maintain and control their sameness. 
B) Living things maintain and control their changelessness. 
C) Living things maintain and control their equilibrium. 
D) Living things maintain and control their disequilibrium. 
E) none of the above

Question 11

The rate of a chemical reaction is inversely proportional to the temperature.

Accepted Answer

A) True 
 B)False

Question 12

Equilibrium involves the ideas of sameness and constancy.

Accepted Answer

A) True 
 B)False

Question 13

Given N2 (g)+ 3 H2 (g)⇌ 2 NH3 (g),which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?

Accepted Answer

A) Place only N2 into a sealed vessel. 
B) Place only H2 into a sealed vessel. 
C) Place only NH3 into a sealed vessel. 
D) All of the above scenarios. 
E) none of the above 
A) Place only N2 into a sealed vessel. 
B) Place only H2 into a sealed vessel. 
C) Place only NH3 into a sealed vessel. 
D) All of the above scenarios. 
E) none of the above

Question 14

We have the following reaction at equilibrium in a flask, CaSO4(s)⇌ Ca2+(aq)+ SO42+(aq)
What will happen to [Ca2+] if additional CaSO4 is added to the flask?

Accepted Answer

A) It will decrease. 
B) It will increase. 
C) It will not change. 
D) Cannot tell with the information provided. 
A) It will decrease. 
B) It will increase. 
C) It will not change. 
D) Cannot tell with the information provided.

Question 15

For the reaction  
what happens to the equilibrium position if the pressure increases?

Accepted Answer

A) shifts to the left 
B) shifts to the right 
C) does nothing 
D) doubles 
E) halves 
A) shifts to the left 
B) shifts to the right 
C) does nothing 
D) doubles 
E) halves

Question 16

What is the molar solubility,(S),of FeS if the   for this substance?

Accepted Answer

A) 1.2 ×   M 
B) 5.9 ×   M 
C) 7.7 ×   M 
D) 3.5 ×   M 
E) none of the above 
A) 1.2 ×   M 
B) 5.9 ×   M 
C) 7.7 ×   M 
D) 3.5 ×   M 
E) none of the above

Question 17

Adding heat to an endothermic reaction causes the reaction to shift to the right.

Accepted Answer

A) True 
 B)False

Question 18

Since the equilibrium constant (Keq)is calculated using the numerical concentrations of reactants and products, Keq can never be a negative value.

Accepted Answer

A) True 
 B)False

Question 19

The equilibrium expression for the reaction:   .

Accepted Answer

A) True 
 B)False

Question 20

What happens to the equilibrium constant when a catalyst is added to the reaction mixture?

Accepted Answer

A) increases 
B) decreases 
C) does not change 
D) varies 
E) none of the above 
A) increases 
B) decreases 
C) does not change 
D) varies 
E) none of the above

What is the value for the for a compound MX(s)if at equilibrium

The equilibrium expression for the reaction: .

For the reaction what happens to the equilibrium position if the volume increases?

Iron(II)carbonate ( = 3.07 × 10^-11)is more soluble than calcium fluoride ( = 1.46 × 10^-10).

As long as K_eq> 1,all reactants will eventually be consumed and leave us exclusively with product molecules.

Which of the following is TRUE of a system for which >> 1?

A reaction that has K_eq = 2.0 × 10^-8 will have high concentrations of products.

A compound with a very large value is generally considered to be only partially soluble.

Decreasing the volume of the system below causes the reaction to shift towards the right.

A description of life is:

The rate of a chemical reaction is inversely proportional to the temperature.

Equilibrium involves the ideas of sameness and constancy.

Given N₂ (g)+ 3 H₂ (g)⇌ 2 NH₃ (g),which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?

We have the following reaction at equilibrium in a flask, CaSO₄(s)⇌ Ca²⁺(aq)+ SO₄²⁺(aq) What will happen to [Ca²⁺] if additional CaSO₄ is added to the flask?

For the reaction what happens to the equilibrium position if the pressure increases?

What is the molar solubility,(S),of FeS if the for this substance?

Adding heat to an endothermic reaction causes the reaction to shift to the right.

Since the equilibrium constant (K_eq)is calculated using the numerical concentrations of reactants and products, K_eq can never be a negative value.

The equilibrium expression for the reaction: .

What happens to the equilibrium constant when a catalyst is added to the reaction mixture?

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Exam 15: Chemical Equilibrium

What is the value for the for a compound MX(s)if at equilibrium

The equilibrium expression for the reaction: .

For the reaction what happens to the equilibrium position if the volume increases?

Iron(II)carbonate ( = 3.07 × 10-11)is more soluble than calcium fluoride ( = 1.46 × 10-10).

As long as Keq> 1,all reactants will eventually be consumed and leave us exclusively with product molecules.

Which of the following is TRUE of a system for which >> 1?

A reaction that has Keq = 2.0 × 10-8 will have high concentrations of products.

A compound with a very large value is generally considered to be only partially soluble.

Decreasing the volume of the system below causes the reaction to shift towards the right.

A description of life is:

The rate of a chemical reaction is inversely proportional to the temperature.

Equilibrium involves the ideas of sameness and constancy.

Given N2 (g)+ 3 H2 (g)⇌ 2 NH3 (g),which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?

We have the following reaction at equilibrium in a flask, CaSO4(s)⇌ Ca2+(aq)+ SO42+(aq) What will happen to [Ca2+] if additional CaSO4 is added to the flask?

For the reaction what happens to the equilibrium position if the pressure increases?

What is the molar solubility,(S),of FeS if the for this substance?

Adding heat to an endothermic reaction causes the reaction to shift to the right.

Since the equilibrium constant (Keq)is calculated using the numerical concentrations of reactants and products, Keq can never be a negative value.

The equilibrium expression for the reaction: .

What happens to the equilibrium constant when a catalyst is added to the reaction mixture?

The Chemical World

Measurement and Problem Solving

Matter and Energy

Atoms and Elements

Molecules and Compounds

Chemical Composition

Chemical Reactions

Quantities in Chemical Reactions

Electrons in Atoms and the Periodic Table

Chemical Bonding

Gases

Liquids, solids, and Intermolecular Forces

Solutions

Acids and Bases

Oxidation and Reduction

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

Iron(II)carbonate ( = 3.07 × 10^-11)is more soluble than calcium fluoride ( = 1.46 × 10^-10).

As long as K_eq> 1,all reactants will eventually be consumed and leave us exclusively with product molecules.

A reaction that has K_eq = 2.0 × 10^-8 will have high concentrations of products.

Given N₂ (g)+ 3 H₂ (g)⇌ 2 NH₃ (g),which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?

We have the following reaction at equilibrium in a flask, CaSO₄(s)⇌ Ca²⁺(aq)+ SO₄²⁺(aq) What will happen to [Ca²⁺] if additional CaSO₄ is added to the flask?

Since the equilibrium constant (K_eq)is calculated using the numerical concentrations of reactants and products, K_eq can never be a negative value.