MATTER AND ENERGY

IT’S WHAT THE WORLD IS MADE OF

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 1
 Objective
• What is matter?
• What are the states of matter?
• What are the properties of matter
• What is Energy?
• Explain the law of the conservation of energy?
• Describe some of the many forms of energy?
• What are the types of energy;

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 2

 What is matter?
• Matter is anything that has mass and takes up
space.

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 3

 STATES OF MATTER
Based upon particle arrangement

Based upon energy of particles

Based upon distance between particles

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 4

 Kinetic Theory of Matter
Matter is made up of particles
which are in continual random
motion.

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 5

 What do you know about matter?

Solids
Gases
Liquids Plasma

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 6

 Solids
• Particles of solids are tightly
packed, vibrating about a
fixed position

• Solids have definite shape

and definite volume.

• Solids have mass.

• Solids take up space.

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 7
 Particles in Solids:
• Are packed tightly
together

• Have very little energy

• Vibrate in place

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 8

 Liquids

• Particles of liquids are

tightly packed, but are far
enough apart to slide over
one another
• Liquids take the shape of
their container and have
definite volume.
• Liquids have mass.
• Liquids take up space.
4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 9
 Particles in Liquids:
• Are loosely packed

• Have medium
energy levels

• Particles flow
around each other

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 10

 Gases
• Particles of gases are
very far apart and move
freely
• Gases spread out to fill
the entire space given
and do not have definite
volume.
• Gases have mass.
• Gases take up space.
4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 11
 Particles in Gases:
• Move freely

• Have LOTS of
energy

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 12

 Plasma
• Lightning is a plasma.
• Used in fluorescent
light bulbs and Neon
lights.
• Plasma is a lot like a
gas, but the particles
are electrically charged.

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 13

 STATES OF MATTER
PLASMA
 A plasma is an
ionized gas.
 A plasma is a very
good conductor of
electricity and is
affected by
magnetic fields.
 Plasmas, like gases • Plasma is the
have an indefinite
common state
shape and an
indefinite volume. of matter

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 14

 PHASE CHANGES
Description of Term for Phase Heat Movement During
Phase Change Change Phase Change

Heat goes into

Solid to Melting the solid as it
liquid melts.
Heat leaves the
Liquid to
Freezing liquid as it
solid
freezes.

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 15

 PHASE CHANGES
Description of Term for Phase Heat Movement During
Phase Change Change Phase Change
Vaporization,
Liquid to which includes Heat goes into the
gas boiling and liquid as it vaporizes.
evaporation
Heat leaves the gas
Gas to liquid Condensation
as it condenses.
Heat goes into the
Solid to gas Sublimation
solid as it sublimates.

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 16

 STATES OF MATTER

SOLID LIQUID GAS PLASMA

Tightly packed, in a Close together with Well separated with Has no definite
regular pattern no regular no regular volume or shape
Vibrate, but do not arrangement. arrangement. and is composed of
move from place to Vibrate, move Vibrate and move electrical charged
place about, and slide freely at high particles
past each other speeds
4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 17
 What are properties?
• Matter has observable and measurable
qualities.
• We can use general properties to identify
substances.
• Two basic types of properties of matter:
Physical properties and Chemical
properties:

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 18

 Physical Properties
• Physical properties are used to identify, describe and
classify matter.
– Characteristic of a substance that can be observed (using
your senses) without changing the substance into
something else.

Hardness Texture Color

Odor Taste Temperature

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 19
 More EXAMPLES - Physical

• size, shape, freezing point, boiling point,

melting point, magnetism, viscosity, density,
luster and many more.
– Viscosity - The resistance of a liquid to flowing.
– Examples:
– Low viscosity-water, rubbing alcohol
– High viscosity-honey

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 20

 Chemical Properties
• Chemical properties are characteristics involved
when a substance interacts with another substance
to change its chemical make-up.

Flammability Rusting Creating gas

bubbles
Creating a new Reactivity with pH
chemical product water

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 21

 Review Questions
1. What state of matter has definite volume and
definite shape?
2. Describe the properties of liquids.
3. Describe the differences between gases and
plasma.
4. What is needed for states of matter to change
phase?

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 22

 Energy
• Energy is defined as the ability of a body or
system of bodies to perform work.
• Energy plays an essential role both in everyday
events and in scientific phenomena;
• Example, energy provided by our foods, to the
energy we use to run our cars, to the sunlight
that warms us on the beach;
• The unit of energy is Joule (J). The Joule is the
work done when a force of one Newton moves
through a distance of 1m;
4/8/2015 FA & JJ /APP PHYS/NURS 106 23
 Nature of Energy
• Energy is all around us:
Energy as sound
Energy as light
Energy as wind
Energy as food

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 24

 Forms of Energy
Electrical
– Kinetic energy associated with the flow of electrical charge.
• Heat or Thermal Energy
– Kinetic energy associated with molecular motion.
• Light or Radiant Energy
– Kinetic energy associated with energy transitions in an atom.
• Nuclear Energy
– Potential energy in the nucleus of atoms.
• Chemical Energy
– Potential energy in the attachment of atoms or because of
their position.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 25

 Law of Conservation of Energy
• The law states that energy can neither be
created nor destroyed but can be transformed
from one form to another;
• The total energy in the universal or a closed
system is constant and can neither be created
nor destroyed;
• All forms of energy can be converted into
other forms.
– The sun’s energy through solar cells can be
converted directly into electricity.

4/8/2015 FA & JJ /APP PHYS/NURS 106 26

 Examples
• Green plants convert the sun’s energy
(electromagnetic) into starches and sugars
(chemical energy).
• In an electric motor, electromagnetic energy
is converted to mechanical energy.
• In a battery, chemical energy is converted
into electrical energy.
• The mechanical energy of a waterfall is
converted to electrical energy in a generator.

4/8/2015 FA & JJ /APP PHYS/NURS 106 27

 Examples
• In an automobile engine, fuel is burned to
convert chemical energy into heat energy.

• The heat energy is then changed into

mechanical energy;

4/8/2015 FA & JJ /APP PHYS/NURS 106 28

 Units of Energy
• Calorie (cal) is the amount of energy needed
to raise one gram of water by 1 °C.
– kcal = energy needed to raise 1000 g of
water 1 °C.
– food calories = kcals.
Energy Conversion Factors
1 calorie (cal) = 4.184 joules (J)
1 Calorie (Cal) = 1000 calories (cal)
1 kilowatt-hour (kWh) = 3.60 x 106 joules(J)
6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 29
 Measurement of Energy

• Converting Calories to Joules

• Express 40.5 cal of energy in units of joules.
Solution
1 cal = 4.184 J 40.5cal  4.184J  169.5J
1

• How many calories of energy correspond to 28.4 J? [6.8

cal]

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 30

 Energy Use

Energy Required to Raise Energy Required Energy Used by

Temperature of 1 g of to Light 100-W Average Person
Unit Water by 1°C Bulb for 1 Hour in 1 Day
joule (J) 4.18 3.6 x 105 9.0 x 108

calorie (cal) 1.00 8.60 x 104 2.2 x 108

Calorie (Cal) 1.00 x 10-3 86.0 2.2 x 105

kWh 1.1 x 10-6 0.100 2.50 x 102

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 31

 Chemical Potential
Energy
• The amount of energy stored in a material is its
chemical potential energy.
• The stored energy arises mainly from the
attachments between atoms in the molecules and the
attractive forces between molecules.
• Chemical reactions happen most readily when
energy is released during the reaction.
• Molecules with lots of chemical potential energy
are less stable than those with less chemical
potential energy.
• Energy will be released when the reactants have
more chemical potential energy than the products.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 32

 Exothermic Processes
• When a change results in the release of energy it is
called an exothermic process.
• An exothermic chemical reaction occurs when the
reactants have more chemical potential energy than the
products.
• The excess energy is released into the surrounding
materials, adding energy to them.
– Often the surrounding materials get hotter from the
energy released by the reaction.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 33

 An Exothermic
Reaction Surroundings

reaction

Reactants

Potential energy
Amount
of
energy
Products released

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 34

 Endothermic Processes
• When a change requires the absorption of energy it
is called an endothermic process.
• An endothermic chemical reaction occurs when the
products have more chemical potential energy than
the reactants.
• The required energy is absorbed from the
surrounding materials, taking energy from them.
– Often the surrounding materials get colder due to
the energy being removed by the reaction.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 35

 An Endothermic
Reaction Surroundings

reaction

Products

Potential energy
Amount
of
energy
Reactants absorbed

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 36

 Energy and the Temperature of
Matter
• The amount by which temperature of an object
increases depends on the amount of heat energy
added (q).
• If you double the added heat energy the
temperature will increase twice as much.
• Temperature increase of an object also depends on
the mass of the object.
• If you double the mass, it will take twice as much
heat energy to raise the temperature the same
amount.
6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 37
 Heat Capacity
• Heat capacity is the amount of heat a substance
must absorb to raise its temperature by 1 °C.
– cal/°C or J/°C.
– Metals have low heat capacities; insulators have
high heat capacities.
• Specific heat = heat capacity of 1 kilogram of the
substance.
– cal/g°C or J/g°C.
– Water’s specific heat = 4.184 J/g°C for liquid.
• Or 1.000 cal/g°C.
• It is less for ice and steam.
6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 38
 Specific Heat Capacity
• Specific heat is the amount of energy required to raise the
temperature of one kilogram of a substance by 1 °C.
• The larger a material’s specific heat is, the more energy it
takes to raise its temperature by a given amount.
• Like density, specific heat is a property of the type of
matter.
– It doesn’t matter how much material you have.
– It can be used to identify the type of matter.
• Water’s high specific heat is the reason it is such a good
cooling agent.
• It absorbs a lot of heat for a relatively small mass.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 39

 Specific Heat Capacities
Substance Specific Heat
J/g°C
Aluminum 0.903
Carbon (dia) 0.508
Carbon (gra) 0.708
Copper 0.385
Gold 0.128
Iron 0.449
Lead 0.128
Silver 0.235
Ethanol 2.42
Water (l) 4.184
Water (s) 2.03
Water (g) 2.02

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 40

 Energy and Energy Changes

Examples:
• When food burns with oxygen, energy in the form of
heat is released, such a process is exothermic.
• When complex molecules such as amino acids,
glycogen and fats in the body are broken down during
an emergency, energy in the form of heat is absorbed.
• Also, the liver uses energy to breakdown drug
molecules in the body into smaller forms.
• Such processes are endothermic processes.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 41

 Examples
Exothermic processes Endothermic processes
• burning sugar • producing sugar by
• rusting iron photosynthesis
• cooking an egg

4/8/2015 JJW, FA & IA /APP CHEM/NURS 107 42

 GAS LAWS:

BOYLE’S
CHARLE’S
AVOGADRO’S
GAY-LUSSAC’S

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 43

 Physical Characteristics of Gases
Physical Characteristics Typical Units
Volume, V liters (L)

Pressure, P atmosphere
(1 atm = 1.015x105 N/m2)
Temperature, T Kelvin (K)

Number of atoms or mole (1 mol = 6.022x1023

molecules, n atoms or molecules)

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 44

 STP
Standard Temperature & Pressure

0°C 273 K

1 atm 101.325 kPa

-OR-

101.325 kPa (kilopascal) = 1 atm = 760 mm Hg= 760

torr = 14.7 psi

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 45

 Boyle’s Law
‘Relating Volume and Pressure’
 Pressure and volume
are inversely related at
constant temperature.
 PV = K
 As one goes up, the other
goes down.
 P1V1 = P2V2
“Father of Modern Chemistry”
Robert Boyle
Chemist & Natural Philosopher
Listmore, Ireland
January 25, 1627 – December 30, 1690

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 46

 Boyle’s Law:
P1V1 = P2V2

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 47

 Boyle’s Law:

P1V1 = P2V2

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 48

 Boyle’s Law

• Boyle's Law is important because it relates

changes in the volume of a gas to changes in
pressure (depth) and defines the relationship
between pressure and volume in breathing gas
supplies.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 49

 Charles’ Law;
‘Relating Volume and Temperature’

 Volume of a gas varies

directly with the absolute
temperature at constant
pressure.
 V = KT
Jacques-Alexandre Charles
 V1 / T1 = V2 / T2 Mathematician, Physicist, Inventor
Beaugency, France
November 12, 1746 – April 7, 1823

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 50

 Charles’ Law:
V1/T1 = V2/T2

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 51

 Charles’ Law:

V1/T1 = V2/T2

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 52

 Charles’ Law Problems

3
• A gas cm
occupies 473 at36°C. Find its
3
volume in cm at 94°C.
• A sample of gas at 15ºC and 1 atm has a
volume of 2.50 L. What volume will this gas
occupy at 30ºC and 1 atm?

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 53

 Avogadro’s Law
Relating Volume and Number of Moles’

At constant temperature

and pressure, the volume of
a gas is directly related to
the number of moles.
V = K n
V1 / n1 = V2 / n2
Amedeo Avogadro
Physicist
Turin, Italy
August 9, 1776 – July 9, 1856

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 54

 Avogadro’s Law:
V1/n1=V2/n2

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 55

 Gay-Lussac Law;
Relating Pressure and Temperature’
 At constant volume, pressure
and absolute temperature are
directly related.
 P= kT
 P1 / T1 = P2 / T2

Joseph-Louis Gay-Lussac
Experimentalist
Limoges, France
December 6, 1778 – May 9, 1850

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 56

 Gay-Lussac's Law

• 10.0 L of a gas is found to exert 97.0 kPa at

25.0°C. What would be the required
temperature (in Celsius) to change the
pressure to standard pressure?
• 5.00 L of a gas is collected at 22.0°C and
745.0 mmHg. When the temperature is
changed to standard, what is the new
pressure?.[0.091]
6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 57
 Problems

• 5.0 g of neon is at 256 mm Hg and at a temperature of 35º

C. What is the volume? Neon-20.1797, R= 0.08206
Latm/mol K [ 18.76 L]
• What is a gas’s temperature in Celsius when it has a volume
of 25 L, 203 mol, 143.5 atm? R= 0.08206 Latm/mol K
[215.40K, 215.40- 273= -57.63 º C]
• Find the volume, in mL, when 7.00 g of O2 and 1.50 g of
Cl2 are mixed in a container with a pressure of 482 atm and
at a temperature of 22º C. [0.0121L = 121mL]

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 58

 Differences Between Ideal and Real Gases
Ideal Gas Real Gas
Obey PV=nRT Always Only at very low
P and high T
Molecular volume Zero Small but not
zero
Molecular attractions Zero Small

Molecular repulsions Zero Small

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 59

 Real Gases
 Real molecules do take up space and do interact with each
other (especially polar molecules).
 Need to add correction factors to the ideal gas law to account
for these.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 60

 Combined Gas Equation

1
V
Boyle’s law ( P ) and Charles’s law ( VT
) can be combined and
expressed in a single statement:
the volume occupied by a given amount of gas is proportional to the
absolute temperature divided by the pressure
( V T ) this equation Can be written as.
P

P1V1 P2 V2

T1 T2

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 61

 Ideal Gases

An “ideal” gas exhibits certain theoretical properties.

Specifically, an ideal gas …
• Obeys all of the gas laws under all conditions.
• Does not condense into a liquid when cooled.
• Shows perfectly straight lines when its V and T & P
and T relationships are plotted on a graph.
In reality, there are no gases that fit this definition
perfectly.
We assume that gases are ideal to simplify our
calculations.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 62

 Ideal Gas Law

• The Ideal Gas Law is simply the combination of Boyle’s

law, Charles’s law, Gay-Lussac’s law, and Avogadro’s
law.
• The ideal gas equation has the following form: PV= nRT
P = pressure in atmospheres (atm)
V = volume in liters (L)
n= moles of gas
T= the temperature in Kelvin (K)
R= the ideal gas constant and is 0.0821 liters atm/K-mol.

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 63

 Ideal Gas Law
PV = nRT
P = Pressure (in kPa) V = Volume (in L)
T = Temperature (in K) n = moles
R = 8.31 kPa • L
K • mol
R is constant. If we are given three of P, V, n,
or T, we can solve for the unknown value.
From Boyle’s Law:
P1V1 = P2V2 or PV = constant
From combined gas law:
P1V1/T1 = P2V2/T2 or PV/T = constant

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 64

 Boyle’s Law Problems
• A volume of air occupying 12.0 dm3 at 98.9 kPa
is com-pressed to a pressure of 119.0 kPa. The
temperature remains constant. What is the new
volume?[9.97dm3]
• A volume of carbon dioxide gas, CO2, equal to
20.0 L was collected at 23C and 1.00 atm
pressure. What would be the volume of carbon
dioxide collected at 23C and 0.830 atm?[]
• Suppose that you have 5.00 liters of a gas at 1.00
atm pressure, and then you decrease the volume to
2.00 liters. What’s the new pressure?

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 65

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 66
 Avogadro's Law Problems
A. 5.00 L of a gas is known to contain 0.965 mol. If the
amount of gas is increased to 1.80 mol, what new volume
will result (at an unchanged temperature and
pressure)?[9.3L]

B. A cylinder with a movable piston contains 2.00 g of helium,

He, at room temperature. More helium was added to the
cylinder and the volume was adjusted so that the gas pressure
remained the same. How many grams of helium were added to
the cylinder if the volume was changed from 2.00 L to 2.70 L?
(The temperature was held constant.)
Molar mass of He= 4g/mol
[]

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 67

 Ideal Gas Law Problems

• A gas has a volume of 675 mL at 35°C and 0.850 atm pressure.

What is the temperature in °C when the gas has a volume of
0.315 L and a pressure of 802 mm Hg?
• A sample of neon gas used in a neon sign has a volume of 15 L at
STP. What is the volume (L) of the neon gas at 2.0 atm and –
25°C?
• Calculate the pressure in atmospheres of 0.412 mol of He at 16°C
& occupying 3.25 L. [3.01 atm ]
• Find the volume of 85 g of O2 at 25°C and 104.5 kPa dm
3
[64 ]

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 69

 Application of Gas Laws
• One practical application of Boyle's law is drawing
fluid into a syringe.
• In respiration Boyles is applicable the volume of the
thoracic cavity increases to reduce pressure in the
cavity thereby allowing air from outside under pressure
to rush into the nostrils.
• This can be used to induce breathing in patients
with breath difficulties.
• Gas expansion can effect equipment designed to hold
gas.
• For instance, anti-shock trousers or MAST suits
(are medical devices used to treat severe blood loss.)

6/23/2016 NURS 105 : LECTURE 2 BY Ms I.A.AGBO 70