Review 15ANS

REVIEW QUESTIONS

Chapter 15

A mixture of 0.10 mol of of and 0.10 mol of is placed in a flask and allowed to reach equilibrium as shown below:

At equilibrium

. Calculate the equilibrium constant,

, for this reaction.


Initial

Equilibrium

At for the reaction shown below:
(A)

Calculate

and

for the reaction shown below:
(B)

At for the following reaction:

In an equilibrium mixture,

and

. What is the concentration of

in the equilibrium mixture?

At for the equilibrium:

If the partial pressures of NOBr and NO are equal at equilibrium, what is the partial pressure of

A mixture of and are place in a 1.00-L flask and allowed to come to equilibrium as shown below. At equilibrium .

a) What are the equilibrium concentrations of

and


Initial

Equilibrium

b) Calculate

and

for this reaction at

When 2.00 mol each of hydrogen and iodine are mixed in a flask, 3.50 mol of HI is produced at equilibrium:

Calculate the equilibrium constant

for this reaction.


Initial

Equilibrium

The equilibrium constant for the reaction

has a numerical value of 3.00 at a given temperature. 1.50 mol each of

and

are mixed in a

flask and allowed to reach equilibrium. What percent of

is converted to product?


Initial

Equilibrium

Taking square root of each side,

Predict how each of the following changes affect the amount of present in an equilibrium mixture in the reaction

a) Raising the temperature of the mixture.

Since reaction is exothermic, raising temperature will shift the equilibrium to the left

and reduce amount of hydrogen.
b) Adding more

Adding more water, will shift the equilibrium to the right

and increase the amount of hydrogen.
c) Doubling the volume of the container holding the mixture.

Increasing the volume of the container will reduce the pressure but the equilibrium will not be affected, and the amount of hydrogen will not change.
d) Adding a catalyst.

Adding catalyst does not alter the equilibrium and the amount of hydrogen produced.
11. At

the equilibrium constant for the reaction below is

. If the initial concentration of NO is 0.500 M , what are the equilibrium concentrations of each substance?


Initial

Equilibrium

Taking square root of each side,

The reaction below has an equilibrium constant . If 0.100 mol of BrCl is placed in a flask and allowed to come to equilibrium, what are the equilibrium concentrations of each substance?


Initial

Equilibrium

Taking square root of each side,

An equilibrium mixture of , and HI at contains and 0.155 M HI in a flask. What are the equilibrium concentrations when equilibrium is reestablished following the addition of 0.100 mol of HI ?

After addition of


Initial

Equilibrium

Taking square root of each side,