Free Printable Chapter 17 and 18 Review

1.

Write the equilibrium constant expression for the following: $N_2\left(g\right)\ +\ O_2\left(g\right)\leftrightarrow\ 2\ NO\ \left(g\right)$

a)

$K_{eq}=\frac{\left[NO\right]}{\left[N_2\right]\left[O_2\right]}$

b)

$K_{eq}=\frac{\left[NO\right]^2}{\left[N_2\right]\left[O_2\right]}$

c)

$K_{eq}=\frac{\left[N_2\right]\left[O_2\right]}{\left[NO\right]}$

d)

$K_{eq}=\frac{\left[N_2\right]\left[O_2\right]}{\left[NO\right]^2}$

2.

When a reaction is exothermic, lowering the temperature will shift the equilibrium to the (a) .

3.

Click on the ways will we be able to shift the equilibrium to the right: $2\ CO\ \left(g\right)\ \leftrightarrow\ C\ \left(s\right)\ +\ CO_2\ \left(g\right)\ +\ heat\$

a)

Decreasing the volume

b)

Decreasing the temperature

c)

Increasing the temperature

d)

Decreasing the pressure

4.

Find the $K_{eq}$ for the following equilibrium $H_2\left(g\right)\ +\ I_2\ \left(g\right)\ \leftrightarrow\ 2HI\ \left(g\right)$

\left[H_2\right]\ =\ 0.0109\ ,\ \left[I_2\right]\ =\ 0.00290\ ,\ \left[HI\right]\ =\ 0.0460

a)

1455.23

b)

140.55

c)

66.90

d)

1256.95

5.

If you increase the temperature of an endothermic reaction, the equilibrium will shift (a)

6.

True or False: If the product gas moles equals reactants gas moles then there is no shift..

a)

True

b)

False

7.

Which is the correct equilibrium constant expression for the following: $CO\ \left(g\right)\ +\ 3H_2\ \left(g\right)\ \leftrightarrow\ CH_4\ \left(g\right)\ +\ H_2O\ \left(g\right)$

a)

$K_{eq}=\frac{\left[CO\right]\left[H_2\right]}{\left[CH_4\right]\left[H_2O\right]}$

b)

$K_{eq}=\frac{\left[CO\right]\left[H_2\right]^3}{\left[CH_4\right]\left[H_2O\right]}$

c)

$K_{eq}=\frac{\left[H_2O\right]\left[CH_4\right]}{\left[CO\right]\left[H_2\right]^3}$

d)

$K_{eq}=\frac{\left[H_2O\right]\left[CH_4\right]}{\left[CO\right]\left[H_2\right]}$

8.

$2\ S\ \left(s\right)\ +\ 5\ F_2\ \left(g\right)\ \leftrightarrow\ SF_4\ \left(4\right)\ +\ SF_6\ \left(g\right)\$
This equilibrium will shift to the right if _____________.

a)

the concentration of $SF_4$ is increased.

b)

the concentration of $SF_6$ is increased

c)

the pressure on the system is increased.

d)

the pressure on the system is decreaed.

9.

What does a value of K_eq greater than 1 mean?

a)

more reactants than products exist at equilibrium

b)

more products than reactants exist at equilibrium

c)

the rate of the forward reaction is high at equilibrium

d)

the rate of the reverse reaction is high at equilibrium

10.

For the reaction to happen, the particles must have a certain amount of energy.

a)

Collision Theory

b)

Activated complex

c)

Activation Energy

d)

Reactants

11.

What type of reaction is this?

a)

Endothermic Reaction

b)

Exothermic Reaction

12.

The Keq = 4.32. Find the [O2], using the following equilibrium equation. [SO2] = 0.590 and [SO3] = 0.260 $2SO_2\left(g\right)\ +\ O_2\left(g\right)\ \leftrightarrow\ 2SO_3\left(g\right)$

a)

0.35

b)

0.0449

c)

0.0540

d)

0.150

13.

Will the equilirbium shift left or right depending on the following stress:

CO(g) + Fe3O4(s) $\leftrightarrow$ CO2(g) + 3FeO(s)

Stress: volume increase

a)

Left

b)

Right

c)

No Shift

14.

Will the following equilibrium shift left or right depending on the following stress:

PCl5(g) $\leftrightarrow$ PCl3(g) + Cl2(g) + heat

Stress: temperature increase

a)

Left

b)

Right

c)

No Shift

15.

What is Entropy?

a)

Energy can be converted or destroyed.

b)

A measure of disorder or randomness of particles that make up a system.

c)

Energy flows from a warmer object to a colder object.

d)

Spontaneous processes always proceed in such a way that entropy of universe increase.

16.

What is the second law of thermodynamics?

a)

Energy can be converted or destroyed.

b)

A measure of disorder or randomness of particles that make up a system.

c)

Energy flows from a warmer object to a colder object.

d)

Spontaneous processes always proceed in such a way that entropy of universe increase.

17.

Frying an egg, is a type of what reaction?

a)

Endothermic

b)

Exothermic

18.

Snow Formation, is a type of what reaction?

a)

Exothermic

b)

Endothermic

19.

If 335 g of water at 65.5 C loses 9750 J of heat, what is the final temperature of the water?

a)

58.54 C

b)

72.46 C

20.

When calculating enthalpy, $\Delta H$ is

a)

$\Delta H_{reac\tan ts\ }-\Delta H_{products}$

b)

$\Delta H_{products\ }-\ \Delta H_{reac\tan ts}$

21.

Solve for ΔG, ΔH = 15.6 kJ, T = 415 K, ΔS = 45 J/K

(a)

22.

If $\Delta G$ is positive, the reaction is _____________________.

a)

Spontaneous

b)

Nonspontaneous

23.

What mass of ammonium chloride (NH4Cl) would you use to prepare 85.0 mL of a 1.20 M solution NH4Cl? The molar mass of ammonium chloride is 53.50 g/mol.

a)

12.16 g

b)

5.46 g

c)

3.47 g

d)

11.71 g

24.

What mass of water must be added to 0.50 mol of glucose to make a solution of 25% by mass? The molar mass of glucose is 180 g/mol.

(a)

25.

A 41.0 mL barium hydroxide solution of molarity 3.41 M is diluted with water to form 279 mL of the solution. Calculate the molarity of the solution.

a)

0.46 M

b)

0.50M

c)

0.75 M

26.

What is the boiling point elevation of a solution containing 17.1 g of sucrose in 100.0 g of water? The molar mass of sucrose is 342 g.

a)

0.26 C

b)

0.47 C

c)

0.39 C

27.

A solution is made by adding water to 35 ml of methanol (CH3OH) until the final volume of the solution is 275 mL. What is the molarity of the methanol in this solution? The density of methanol is 0.792 g/mL. The molar mass of methanol is 32.04 g/mol.

(a)

28.

Name three factors that increase the rate at which a substance dissolves.

4 lines

29.

Calculate the mole fraction of HCl in an aqueous solution that contains 33.6% by mass. The molar mass of HCl is 36.05 g/mol. The molar mass of water is 18.02 g/mol.

a)

0.40

b)

0.42

c)

0.36

d)

0.20

30.

Convert 126 nutritional calories to joules.

(a)

Chapter 17 and 18 Review

Total questions: 30

Worksheet time: 44mins

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