# Chapter 15 Test...And Then Some

23 Questions | Total Attempts: 167  Settings Create your own Quiz • 1.
Units for equilibrium constants are conventionally omitted because they vary from reaction to reaction.  If they were to be included, the units on Keq for this reaction would be:
• A.

Atm

• B.

1/atm

• C.
• D.

All units would cancel out

• 2.
At 150 degrees Celsius the equilibrium constant for the reaction below has a value of 300.  The reaction was allowed to reach equilibrium in a sealed container and the partial pressure due to IBr (g) was found to be 3 atm.  Which of the following could be the partial pressure due to the Br2 (g) and I2 (g) in the container?
• A.

A

• B.

B

• C.

C

• D.

D

• E.

E

• 3.
Consider a system at equilibrium based on the reaction above.  In such a system, the concentration of oxygen gas is:
• A.

Constant and equal to the concentration of ozone gas

• B.

Constant and less than the concentration of ozone gas

• C.

Constant and greater than the concentration of ozone

• D.

Increasing and the concentration of ozone is increasing

• E.

Increasing and the concentration of ozone is decreasing

• 4.
Given that the Keq for the reaction,  , is 36.  What will be the value for the following reaction:
• A.

36

• B.

18

• C.

6

• D.

1/6

• E.

1/36

• 5.
Which of the following concentration vs. time graphs represents the reaction:
• A.

A

• B.

B

• C.

C

• D.

D

• 6.
Solids are not included in an equilibrium expression because:
• A.

Their concentrations are all 1.0 M and drop out

• B.

Adding more solid does not change the density (concentration of the solid

• C.

Adding more solid does not change the surface area of the solid

• D.

Equilibrium reactions are usually balanced with the lowest hole numbers

• E.

Solids no longer continue to dissolve once the solution because saturated

• 7.
When the system is at equilibrium:
• A.

No further reaction occurs in either direction

• B.

The concentrations of reacts and products are equal

• C.

Forward and reverse reactions are still taking place

• D.

All reactants have been consumed

• 8.
Which equilibrium system would have the following expression for Kc:
• A.
• B.
• C.
• 9.
Consider the equilibrium reaction: What will be the effect of halving the concentration of sulfur trioxide?
• A.

Sulfur dioxide and oxygen will increase equally

• B.

Sulfur increases more than oxygen

• C.

Sulfur dioxide and oxygen decrease equally

• D.

Sulfur dioxide decreases more than oxygen

• E.

Oxygen decreases more than sulfur dioxide

• 10.
At 2000 K, the value of Kc is  for the reaction:
• A.

There is more product present than the reactant

• B.

There is more reactant present than product

• C.

There is a 50/50 mix of reactant and product

• D.

• 11.
Raising the temperature of a system which has reached equilibrium:
• A.

Changes the value of K

• B.

Increases the kinetic energy of the system

• C.

Causes an increase in concentration of reactants for an exothermic reaction

• D.

All of the above

• E.

More than one of the above, but not all of the above

• 12.
If the equilibrium constant for this reaction is 100, what will happen to a mixture in which all species are initially 0.01 M?
• A.

Reaction goes tot he right

• B.

Reaction goes left

• C.

No changes occur, reaction is at equilibrium

• D.

Cannot predict

• 13.
Which must be true of the equilibrium concentrations when 0.10 mole of each reactant are added to an empty 1.0 L container and allowed to reach equilibrium?
• A.

[NO]

• B.

[NO]>[O2]

• C.

[NO]=[O2]

• D.

[NO]=[NO2]

• E.

[NO2]=2[O2]

• 14.
Consider the reaction: the yield of PCl5 could be increased by.
• A.

Adding Ne gas at constant total pressure

• B.

Increasing the temperature

• C.

Removing the Cl2 from the system

• D.

• E.

Reducing the volume of the system

• 15.
For the reaction: 1.0 mole of Fe and 0.50 moles of oxygen are mixed together, reacted and allowed to come to equilibrium in a 1.0 L container.  At equilibrium, 0.20 moles of Fe2O3 have formed.  What is the Keq at this temperature?
• A.
• B.
• C.
• D.
• E.
• 16.
The graph shows the variation of concentration with time for the reaction at 25 degrees Celsius. What is the value of the equilibrium constant, K, at this temperature?
• A.

0.667

• B.

0.845

• C.

1.19

• D.

2.67

• 17.
The quantities which are equal in an equilibrium system are
• A.

Forward and reverse reaction rates

• B.

Amounts of products and reactants

• C.

The forward and reverse rate constants

• D.

Forward and reverse activation

• E.

All of the above

• 18.
As a catalyst is added to a system at equilibrium, the value of the equilibrium constant
• A.

Decreases

• B.

Increases

• C.

Stays the same

• 19.
The Ksp for PbCl2 is 1.6x106-5.  of the following choices which is the greatest amount of Pb(NO3)2 that can be added to 1.0 L of 0.010 M NaCl solution at constant temperature without causing precipitation to occur.
• A.

0.0004 mol

• B.

0.0015 mol

• C.

0.0080 mol

• D.

0.15 mol

• 20.
What is the hybridization of orbitals in the ammonia molecule (NH3)?
• A.

Sp

• B.

Sp2

• C.

Sp3

• D.

Dsp3

• E.

D2sp3

• 21.
Consider the chemical bonds found in solid sodium hydrogen carbonate.  For each bond specified, choose the best description of the bond type. a.  ionic bond b.  hydrogen bond c.  single covalent bond d.  double covalent bond e.  resonance covalent bond with bond order between 1 and 2 Carbon/Oxygen
• A.

A

• B.

B

• C.

C

• D.

D

• E.

E

• 22.
Consider the chemical bonds found in solid sodium hydrogen carbonate.  For each bond specified, choose the best description of the bond type. a.  ionic bond b.  hydrogen bond c.  single covalent bond d.  double covalent bond e.  resonance covalent bond with bond order between 1 and 2 Sodium/Hydrogen carbonate bond
• A.

A

• B.

B

• C.

C

• D.

D

• E.

E

• 23.
Consider the chemical bonds found in solid sodium hydrogen carbonate.  For each bond specified, choose the best description of the bond type. a.  ionic bond b.  hydrogen bond c.  single covalent bond d.  double covalent bond e.  resonance covalent bond with bond order between 1 and 2 oxygen/hydrogen bond
• A.

A

• B.

B

• C.

C

• D.

D

• E.

E

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