Wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Equilibrium and Rates of Chemical Reactions

Total questions: 33

Worksheet time: 55mins

Name
Class
Date
1.

N2 + 3H2 <------>2 NH3 + heat

An increase in temperature will produce

a)

more NH3

b)

less NH3

c)

a shift to the right

d)

less N2

2.

H2 + I2 <-------> 2HI

What is the Keq of the following reaction, if the concentrations at equilibrium are [H₂]=0.7, [I₂]=0.3 and [HI]=0.6?

a)

1.7

b)

0.5

c)

2.9

d)

0.15

3.

If the Keq = 0.65

a)

the forward reaction is favored

b)

the reverse reaction is favored

c)

not enough information is given

4.

2 H2S <------> 2 H2 + S2

When the contents were analyzed they were 0.6 mole of H₂S and 0.80 mole S₂ in a 1L container and Keq = 0.016. What is the concentration of H2?

a)

0.007

b)

0.08

c)

0.04

d)

0.2

5.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
6.

Which of the following is true about chemical reaction at equilibrium

a)

only the forward reaction stops

b)

only the reverse reaction stops

c)

both forward and reverse reactions stop

d)

the rate constants for the forward and reverse reactions are equal

e)

the rates of the forward and reverse reactions are equal

7.
Which of the two graphs reaches equilibrium?
a)
The left one.
b)
The right one.
c)
Both of them.
d)
Neither.
8.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
9.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
10.

Which of the following is NOT true at equilibrium?

a)

The forward and reverse reactions proceed at the same rate.

b)

The amount (concentration) of reactants and products do not change.

c)

The amount (concentration) of the reactants is equal to the concentration of the products.

d)

The forward and reverse reactions continue to occur.

11.

For the graph, choose the CORRECT statement.

a)

The rate of reaction slowly increase

b)

The systems never reach equilibrium

c)

At equilibrium, more NO2 is present than N2O4.

d)

At start of reaction, only NO2 was present.

12.

Which of the following statements is CORRECT for a reaction at an equilibrium?

a)

The rate of forward and reverse reactions are equal.

b)

The final concentrations of product and reactant are equal.

c)

The initial concentrations of product and reactant are equal.

d)

The rate constant of the forward and reverse reactions are equal.

13.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
14.
Which of the following shows the correct dissolution reaction for BaCl2?
a)
Ba 2+(aq) + Cl2-(aq) -> BaCl2(s)
b)
BaCl2(aq) -> Ba 2+(aq) + 2Cl-(aq)
c)
 BaCl2(s) -> Ba 2+(aq) + 2Cl-(aq)
d)
Ba 2+(aq) + 2Cl-(aq) -> BaCl2(s)
15.
At what time does the reaction reach equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
16.

N2(g) + 3H2(g) ↔ 2 NH3(g) + heat

Adding H2 will cause the equilibrium to:

a)

Shift right

b)

Shift left

c)

Have no change

d)

Speed up

17.

Why are solids eliminated from the Keq expression?

a)

The abbreviated form is easier to use

b)

They take no visible part in the reaction

c)

The concentration is constant

d)

The concentration is zero

18.

We recognize the existences of equilibrium by observing

a)

The equilibria are dynamic

b)

A consistency of macroscopic properties

c)

Stresses can cause change

d)

A static state of microscopic properties

19.

In an equilibrium expression, the reactants

a)

appear in the denominator

b)

are multiplied by the products

c)

are part of the numerator

d)

are in solid state

20.

When a state of equilibrium between two opposing chemical reactions is reached:

a)

both reactions continue but the net chance is zero

b)

the reaction stops

c)

50% of the original reactants have been changed into the final products

d)

the rates of the opposing reactions are no longer equal

21.

2SO2 (g) + O2 --> 2SO3 (g) + heat

Which of the following stressed on the system will maximize the yeild of SO3?

a)

remove O2

b)

adding a catalyst

c)

increase pressure

d)

increase temperature

22.

PbCO3 (s) --> Pb (aq) + CO3 (aq)

If the Ksp value for PbCO3 is 7.4x10^-14, what is the solubility

a)

3.6x10^6 M

b)

2.7 x10^-7 M

c)

3.7x10^-14 M

d)

7.4 x10^-14 M

23.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

24.

For the reaction...

SO2 + O2 ⇌ SO3

If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.

a)

left

b)

right

c)

left and right

d)

neither left nor right

25.

For the reaction...

N2 (g) + 3 H2(g) ⇌ 2 NH3 (g)


If the pressure in the system is increased, which substance(s) will increase in concentration?

a)

N2

b)

H2

c)

N2 and H2

d)

NH3

26.
If the equilibrium constant is much greater than one (K >> 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
27.
If the equilibrium constant is much less than one (K << 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
28.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2/[N2O4]
b)
Kc = [N2O4]/[NO2]2
c)
Kc = [N2O4]2/[NO2]
d)
Kc = [NO2]/[N2O4]2
29.
What is the equilibrium-constant expression for 
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
a)
Kc= [CO][H2O] / [CO2][H2]  
b)
Kc= [CO2][H2] / [CO]
c)
Kc= [CO2][H2] / [CO][H2O]
d)
Kc= [CO] / [CO2][H2]  
30.

The Ksp expression for a saturated solution of Ca3(PO4)2 is

a)

Ksp = [Ca2+][PO43-]

b)

Ksp = [3Ca2+][2PO43-]

c)

Ksp = [Ca2+]3[PO43-]2

d)

Ksp = [3Ca2+]3[2PO43-]2

31.

The molar solubility of silver sulphide is 5.0 x 10-17 mol/L. Calculate its solubility product.

a)

Ksp = 5 x 1049

b)

Ksp = 5 x 1033

c)

Ksp = 5 x 10-49

d)

Ksp = 5 x 10-33

32.

What will happen if some solid AgNO3 is added to a saturated solution of AgCl ?

a)

The AgNO3 will not dissolve

b)

More solid AgCl will dissolve

c)

More solid AgCl will produced

d)

There will be no effect on AgCl equilibrium

33.

A person mixes 100.0 mL of 0.0015M CaCl2 and 50.0 mL of 0.0081M K2SO4. If the Ksp for CaSO4 is 2.4 x 10-5 , will a CaSO4 precipitate be observed?

a)

No precipitate occur

b)

Precipitate occur

Similar Resources on Wayground

PTS PROYEK IPAS KELAS X

30 questions

PTS PROYEK IPAS KELAS X

quiz

Worksheet

•

12th Grade - University

Summative Test Review SOL 6.8 e,d,g,h

36 questions

Summative Test Review SOL 6.8 e,d,g,h

quiz

Worksheet

•

6th - 12th Grade

Form 5_Ch 21

28 questions

Form 5_Ch 21

quiz

Worksheet

•

9th - 12th Grade

Life cycle of a human

28 questions

Life cycle of a human

quiz

Worksheet

•

3rd Grade - University

Magnetism and Electricity

28 questions

Magnetism and Electricity

quiz

Worksheet

•

KG - Professional Dev...

Naming Organic Compounds Practice

29 questions

Naming Organic Compounds Practice

quiz

Worksheet

•

12th Grade

random stuff (with bots)

28 questions

random stuff (with bots)

quiz

Worksheet

•

KG - Professional Dev...

5 Md 1

28 questions

5 Md 1

quiz

Worksheet

•

8th Grade - University