1. HT1 01 – Introduction to Energy, heat, and temperature
Unit 04 - Heat
HT1 01 – Introduction to Energy, heat, and temperature

2. The Concept of Energy
Although you may know what energy is, it may be difficult to define it.
Energy:
the ability to do work or produce heat.
What forms can energy come in?
Light energy, nuclear energy, and electrical energy
Biomass, petroleum, natural gas, and coal are examples of stored chemical energy
Chemical energy is converted to thermal energy (heat) when we break those bonds
In this unit, we will focus on heat energy.

3. Potential & Kinetic Energy
Energy of motion
i.e.:
a rock rolling down a hill has kinetic energy
Atoms and molecules have kinetic energy as they are always in motion
Potential Energy
Energy that is stored in something, and has the potential to do work, is called potential energy.
a rock sitting at the top of a hill has potential energy

4. Potential Energy – Chemical Bond Energy
This energy exists because of the attractive forces between molecules and atoms.
It plays a large part in chemical reactions.
Therefore, the bonds that hold molecules together are stored energy and may do work (or give off heat) if they are broken.

5. The Law of Conservation of Energy
The Law of Conservation of Energy states that energy cannot be created or destroyed, but only change forms.
This law is also known as the First Law of Thermodynamics.
i.e.:
When octane (C3H8, the main component of gasoline) is burned in your car engine, chemical bond energy (potential energy) is converted into mechanical energy (pistons moving in the car engine; kinetic energy) and heat.
When we eat, our bodies convert the chemical energy of the food into movement of our muscles; again heat is also a product of this conversion.
When we turn on a light switch, electrical energy is converted into light energy and, you guessed it, heat energy.
When talking about chemical reactions, all the energy in the reaction must come from somewhere. That is, it is not spontaneously created.
The only place that energy is stored is in the bonds between atoms.
This potential bond energy will usually be converted to kinetic energy (heat).

6. Kinetic Molecular Theory
Previous science courses may have taught us that molecules in a substance, no matter its state, are in constant motion.
Molecules move slowest in solids, faster in liquids, and fastest in gasses.
The energy a particle has because of its motion is called kinetic energy.
The energy associated with the movement of particles is called heat and thermal energy.
What happens to the motion of particles as they are the temperature of a substance is increased?
Since the particles begin to move faster, then they have more kinetic energy. Therefore, the heat an object gives off is directly related to the motion of its particles.

7. Heat – A TRANSFER of Energy
Heat is the transfer of energy. Note that heat always flows from hot to cold, never from cold to hot.
For example, imagine you had an ice cube in your hand. The heat from your hand gets transferred to the ice cube.
That is, fast moving particles hit the slow moving particles in the ice cube.
This interaction slows the particles down in your hand (making it cold) and speeds up the particles in the ice (making it warm).
Thus, thermal energy is transferred from your hand into the ice cube (coldness does not travel from the ice cube to your hand).
If you were holding a cold piece of metal (instead of ice) your hand will eventually warm the metal to the same temperature as your body.
At this point your hand and the metal are in thermal equilibrium.

8. Heat
Heat:
Internal energy transferred from one thing to another due to a temperature difference
Internal energy in transit
Heat is a form of energy. It is the total amount of kinetic energy in a sample of matter.
Heat also flows from a warmer object to a cooler object.
Therefore, the feeling of getting colder is not “coldness” entering your body, but heat (energy) leaving your body.
The S.I. unit for heat is the Joule (J).

9. Forms of Heat Transfer
3 types;
Conduction
Convection
Radiation

10. Radiation
There are no particles between the Sun and the Earth so it MUST travel by radiation
RADIATION ?
How does heat energy get from the Sun to the Earth?

11. Radiation
The transfer of heat in rays, from a hot object, without needing a medium to pass through
Electro Magnetic radiation infrared frequencies (not visible)
It travels in all directions from a hot object
The hotter an object is, the more heat it will radiate out

12. Conduction
Transfer of heat is through a SOLID by being passed from one particle to the next
Requires contact
Particles at the warm end move faster and this then causes the next particles to move faster and so on.
e.g: poker in fire or spoon in tea
In this way heat in an object travels from: the HOT end the cold end

13. Conduction
When you heat a metal strip at one end, the heat travels to the other end.
As you heat the metal, the particles vibrate, these vibrations make the adjacent particles vibrate, and so on and so on, the vibrations are passed along the metal and so is the heat. We call this? Conduction

14. Convection
The transfer of heat by the physical movement of more energetic particles from one location to another.
It is the way in which particles in a GAS or LIQUID move upwards, carrying heat with them
Think about when you boil water, the bubbles move upwards
Or think of a heater in the room, the heat rises around the room

15. Convection Convection current Cooler water sinks Hot water rises
Cools at the surface
Convection current
Cooler water sinks
Hot water rises

16. Three forms of Heat Transfer

17. Heat - Calories: Another way to measure heat energy
A thermochemical “calorie” is defined as:
the amount of heat required to raise the temperature of one gram of water by one degree Celsius (1°C).
Units for calories are written as “cal”
To convert between joules and calories, use the following conversion factors:
1 J = cal and/or
1 cal = J
Examples:
Convert 8181 joules to calories
Convert 2019 calories to joules
Convert 1125 kJ to calories
Convert 4307 kcal to joules

18. Heat - Food for Thought…
Be careful – dietary calories can be deceiving:
A dietary calorie (as written on food labels), written with a big C ( not “cal”) is actually a kilocalorie, or 1000 calories.
What this means is when you look at a label and it says “100 calories per serving!” it really means:
100 C x 1000 cal = cal per serving
1 C

19. Temperature Temperature:
is a measure of the average kinetic energy of a sample of matter. It is the intensity of heat energy.
There are two ways we will measure temperature:
1. Celsius scale based on the freezing and boiling points of water.
2. Kelvin scale based on energy.
The Kelvin scale has no negative numbers. In fact, the lowest temperature that can ever be reached is absolute zero (0 K).
At this temperature, a particle has no energy, and thus, all movement is ceased.
To converge between degrees Celsius and degrees Kelvin, we will use:
K = ˚C where:
K = degrees in Kelvin
˚C = degrees in Celsius
Examples:
Convert 25oC to Kelvin
Convert -35oC to Kelvin
Convert 187 Kelvin to Celsius

20. Heat vs. Temperature
In terms of heat, or energy, an iceberg would have more than a boiling cup of coffee.
Although the temperature of the boiling water is much higher than the iceberg, the iceberg has more particles. Thus, it will have a higher total energy.
A good way to think of temperature is the intensity of heat.
The coffee will have a more intense heat than the iceberg.