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States of Matter and Thermochem review

Total questions: 56

Worksheet time: 46mins

Name
Class
Date
1.
Are particles of matter always in motion?
a)
yes
b)
no
2.
The motion energy of particles is called...
a)
kinetic energy
b)
connecting energy
c)
electrostatic energy
d)
gravitational energy
3.
Temperature is a measure of particle...
a)
kinetic energy
b)
size
c)
colour
d)
electrostatic force
4.
Absolute zero is the temperature (in Kelvin), at which, only in theory...
a)
all particles stop moving
b)
time stands still
c)
space and time merge
d)
energy goes to infinity
5.

Collisions in which particles transfer all their kinetic energy to other particles are called ___.

a)

elastic

b)

inelastic

6.
What is the difference between particles in a gas and a solid?
a)
gas particles are closer together
b)
solid particles move faster than gas particles
c)
solid particles expand on heating
d)
gas particles have more kinetic energy than solid particles
7.

760 mmHg is equal to

a)

1 torr

b)

760 atm

c)

760 torr

d)

101 Pa

8.

A gas is at a pressure of 95 kPa. What is its pressure in atmospheres?

a)

1.5 atm

b)

1.09 atm

c)

0.94 atm

d)

0.82 atm

9.

What does STP (standard temperature and pressure) stand for?

a)

0.0 degree Celcius and 1 atm

b)

1.0 mmHg and 273 degree Kelvin

c)

1.0 degree Celcius and 0 atm

d)

1.0 atm 273 degree Celcius

10.

How many mm Hg is a pressure of 1.05 atm?

a)

529 mm Hg

b)

798 mm Hg

c)

104.8 mm Hg

d)

760 mm Hg

11.
As pressure decreases, boiling point___
a)
decreases
b)
increases
c)
decreases then increases
d)
increases then decreases
12.

According to the reference table, what is the boiling point of ethanoic acid at 80 kPa?

a)

28 oC

b)

100oC

c)

111oC

d)

125oC

13.

Which liquid has the highest vapor pressure at 75oC?

a)

ethanoic acid

b)

ethanol

c)

propanone

d)

water

14.
Liquids with weak intermolecular forces
a)
contain a lot of kinetic energy
b)
easily evaporate
c)
cannot diffuse
d)
freeze easily
15.

Define the term allotropes

a)

Atoms with same proton number but different number of neutrons

b)

Atoms with same proton number but different mass number

c)

Atoms in different arrangement but same structure

d)

Atoms in different arrangement and different structural form

16.
Which consists of carbon atoms?
a)
graphite
b)
diamond
c)
fullerene
d)
all of these
17.

What letter on the diagram represents a gas?

a)

A

b)

B

c)

C

d)

D

18.

What letter on the diagram represents a solid?

a)

A

b)

B

c)

C

d)

D

19.

What letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

D

20.

What is the boiling point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

21.

What is the phase change of a solid to a liquid?

a)

freezing

b)

melting

c)

boiling

d)

condensation

22.
Change from Gas to Solid is called........
a)
Sublimation
b)
Deposition
c)
Fusion
d)
condensation
23.
What is sublimation?
a)
phase change between solid and liquid
b)
pahse change from gas to solid
c)
phase change from solid to gas
d)
phase change from solid to solid
24.

Is the substance gaining or losing energy?

a)

Gaining

b)

Losing

25.

Is the substance gaining or losing energy?

a)

Gaining

b)

Losing

26.

What is happening to the particles in the substance between points D and E?

a)

Melting

b)

Freezing

c)

Vaporizing

d)

Sublimating

27.

What is happening to the particles in the substance between points A and B?

a)

Melting

b)

Freezing

c)

Speeding Up

d)

Slowing Down

28.

What state/phase is the object likely from points A to B?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

29.

Where on the graph are phase changes taking place?

a)

1

b)

2

c)

3

d)

4

e)

5

30.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

31.
If the specific heat of water is 4,186 J/kg∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? 
a)
-80,371.2 J
b)
44,938.6 J
c)
80,371.2 J
d)
112,575.9 K
32.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of  0.10 J/g°C, what is the mass of the iron sample?
a)
25 g
b)
30 g
c)
20 g
d)
50 g
33.
What is the symbol for Thermal Energy?
a)
Q
b)
T
c)
m
d)
Cp
34.
Heat transfers from an area of ____temperature to an area of ___ temperature.
a)
high to low
b)
low to high
c)
high to high
35.

Convert

 450 K450\ K  to Celsius

a)

 723oC723^oC  

b)

 277oC277^oC  

c)

 177 oC177\ ^oC  

d)

 623oC623^oC  

36.

Convert

 0oC0^oC  to Kelvin

a)

 −273 K-273\ K  

b)

 273 K273\ K  

c)

 32 K32\ K  

d)

 −32 K-32\ K  

37.

Which of the following examples is an endothermic reaction?

a)

Potassium Chloride dissolves in water the temperature drops.

b)

Acid mixed with Sodium Carbonate the temperature drops.

38.

In an endothermic reaction, energy is _________.

a)

absorbed

b)

released

39.
When water is heated from 10°C to 15°C What is the change in temperature?
a)
10 °C
b)
5 °C
c)
15 °C
d)
25 °C
40.
When a  piece of aluminum foil is taken out of the oven and cools from 100°C to 50°C.
What is the change in temperature?
a)
50°C
b)
0°C
c)
100°C
d)
150°C
41.
Calculate the amount of energy required to melt 35.0 grams of ice.
(not in sig figs)  Hf = 80.0 cal/g,  Hv = 560.0 cal/g, SH = 1.00 cal/g ºC
a)
19,600 cal
b)
35.0 cal
c)
2,800 cal 
d)
1,568,000 cal 
42.
How much energy is required to completely boil away 150g of 10o C water? Use C = 4.184 J/goC for water, and Hv = 2260 J/g.
a)
56,484 J
b)
339,000 J
c)
395,484 J
d)
385,484 J
43.
If a 8.50g ice cube at -10o C sits out on the counter, completely melts, and then warms to room temperature (25o C) how much energy did the ice cube absorb? Use C = 2.108 J/goC for ice, C = 4.184 J/goC for water, and Hf = 334 J/g.
a)
179.18 J
b)
2839 J
c)
889.1 J
d)
3907.3 J
44.

The following equation shows the reaction between  Ag+Ag^+  and  Cl−Cl^-  ions.
 Ag+Ag^+  +  Cl−Cl^-  -> AgCl    Δ\Delta H= -65 kJmol−1kJmol^{-1}  
Which of the following is true about the above equation?

a)

Exothermic reaction occurs

b)

Heat is absorbed from the surrounding

c)

The energy content of the reactants is less than the products

d)

65 kJ of heat is absorbed when 1 mole of silver chloride is formed

45.

A chemical reaction that absorbs heat from the surroundings is said to be __________ and has a __________ΔH at constant pressure

a)

endothermic; positive

b)

endothermic; negative

c)

exothermic; negative

d)

exothermic; positive

46.
What letter represents the energy of the products?
a)
A
b)
B
c)
C
d)
D
47.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
48.
Is this reaction endothermic or exothermic?
a)
endothermic 
b)
exothermic
49.

What is the ΔH of this reaction?

a)

40 kJ

b)

20 kJ

c)

80 kJ

d)

-60 kJ

50.
What is the activation energy?
a)
40 kJ
b)
20 kJ
c)
100 kJ
d)
60 kJ
51.
Which letter represents the activation energy?
a)
B
b)
E
c)
C
d)
D
52.

What is the change of the heat of the reaction (ΔH)?

a)

100 kJ

b)

-175 kJ

c)

-50 kJ

d)

75 kJ

53.

Using the equations below:


C(s) + O2(g) → CO2(g) ∆H = –390 kJ

Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ


what is ∆H (in kJ) for the following reaction?


MnO2(s) + C(s) → Mn(s) + CO2(g)

a)

910

b)

130

c)

-130

d)

-910

54.

Consider the following equations.


Mg(s) + O2(g) → MgO(s) ∆H = –602 kJ

H2(g) + O2(g) → H2O(g) ∆H = –242 kJ


What is the ∆H value (in kJ) for the following reaction?


MgO(s) + H2(g) → Mg(s) + H2O(g)

a)

-844

b)

-360

c)

+360

d)

+844

55.

Hess' Law makes use of which principle to calculate the enthalpy change of a reaction?

a)

The law of conservation of energy

b)

The law of conservation of matter

c)

The law that you will always find a lost item in the last place you look for it

d)

Murphy's law

56.

The standard enthalpy change of formation values of two oxides of phosphorus are:


P4(s) + 3O2(g) → P4O6(s) ΔHf = –1600 kJ mol–1

P4(s) + 5O2(g) → P4O10(s) ΔHf = –3000 kJ mol–1


What is the enthalpy change, in kJ mol–1, for the reaction below?


P4O6(s) + 2O2(g) → P4O10(s)

a)

+4600

b)

+1400

c)

–1400

d)

–4600

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