Chapter 9 “Heat” Honors Physics. Temperature Adding or removing energy changes the temperature. Temperature is the average KE of the atoms and molecules.

Chapter 9 “Heat”

Honors Physics

Temperature

• Adding or removing energy changes the temperature.

• Temperature is the average KE of the atoms and molecules present. High avg. KE = high temp.

• We use relative scales: ºF , ºC and absolute scales: K

Temperature

• Internal energy (ΔU) is the energy associated with atomic motion and is proportional to the substance's temperature.

• Temperature is changed by adding or removing energy.

Temperature

Celsius-Fahrenheit Temperature

Conversions

Tf = 9/5 Tc + 32.0

Celsius-Kelvin Temperature

Conversions

T = Tc + 273.15

Concept Check

The lowest outdoor temperature ever

recorded on Earth is -128.6°F,

recorded at Vostok Station,

Antarctica in 1983. What is this

temperature on the Celsius and

Kelvin scales?

Concept Check

-89.2° C, 184 K

Concept Check

The temperatures of one

northeastern state range from 105° F

in the summer to -25°F in the winter.

Express this temperature range in

degrees Celsius and in kelvins.

Concept Check

41°C to -32°C, 314 K to 241 K

Concept Check

A pan of water is heated from 23°C to

78°C. What is the change in its

temperature on the Kelvin and

Fahrenheit scales?

Concept Check

55 K, 99°F

Concept Check

Liquid nitrogen is used to cool

substances to very low temperatures.

Express the boiling point of liquid

nitrogen (77.34 K at 1 atm of

pressure) in degrees Celsius and in

degrees Fahrenheit.

Concept Check

-195.81°C, -320.5°F

Heat

• Heat is the energy transferred between objects due to the difference in their temperatures.

• Heat will naturally go from objects of high KE to objects of low KE. To go in the opposite direction requires work.

Thermal (Heat) Units

• We’ll be mostly using joules (J) or calories (cal). However, you should be aware that there are others (p 307).

• 1 calorie is equal to the amount of energy required to heat 1 gram of water from 4º to 5 ºC.

• 1 cal = 4.184 J

Total energy is conserved.

• Conservation of energy states that the sum of the change in the potential energy and the change in kinetic energy and the change in internal energy must equal zero.

PE + KE + U = 0

Concept Check

Consider an arrangement similar to the one used to demonstrate energy

conservation on p.310. If a total mass of 11.5 kg falls 6.69 m and all

of the mechanical energy is converted to internal energy, by how much will the internal energy of the

water increase?

Concept Check

755 J

Concept CheckA worker drives a 0.500 kg spike into

a rail tie with a 2.50 kg sledgehammer. The hammer hits the

spike with a speed of 65.0 m/s. If one-third of the hammer's kinetic

energy is converted to the internal energy of the hammer and spike, how much does the total internal

energy increase?

Concept Check

1.76 x 103 J

Concept Check

A 3.0 x 10-3 kg copper penny drops a distance of 50.0 m to the ground. If 65% of the initial potential energy goes into increasing the internal

energy of the penny, determine the magnitude of that increase.

Concept Check

0.96 J

Concept Check

The amount of internal energy needed to raise the temperature of

0.25 kg of water by 0.2ºC is 209.3 J. How fast must a 0.25 kg baseball

travel in order for its kinetic energy to equal this internal energy?

Concept Check

41 m/s

Calorimetry

• We can calculate the amount of the change in internal energy through calorimetry.

• The equation Q = mct is used.• Q = internal energy change• m = mass• Cp = specific heat (unique)t = change in temperature.

Heat lost = Heat gained

• In an insulated situation (no heat escapes into the surroundings):

Q lost = Q gained

•m1cp1t1 = -m2cp2t2

Calorimetry

• Generally, we use water as the substance that gains the heat since the specific heat of water is known.

Concept Check

What is the final temperature when a 3.0 kg gold bar at 99ºC is dropped

into 0.22 kg of water at 25ºC? (Use the table on p.314.)

Concept Check

47ºC

Concept Check

A 0.225 kg sample of tin initially at 97.5ºC is dropped into 0.115 kg of

water. The initial temperature of the water is 10.0ºC. If the specific heat capacity of tin is 230 J/kg*ºC, what is the final equilibrium temperature of

the tin-water mixture?

Concept Check

18ºC

Concept Check

Brass is an alloy made from copper and zinc. A 0.59 kg brass sample at

98.0ºC is dropped into 2.80 kg of water at 5.0ºC. If the equilibrium temperature is 6.8ºC, what is the specific heat capacity of brass?

Concept Check

390 J/kg*ºC

Concept Check

A hot, just minted copper coin is placed in 101 g of water to cool. The

water temperature changes by 8.39ºC, and the temperature of the

coin changes by 68.0ºC. What is the mass of the coin?

Concept Check

135 g

Phase Changes

• Phase changes occur when an object goes from one phase of matter to another.

• When an object is going through a phase change, added energy is used to make the change without raising the temperature. This is latent heat.

Equations for Phase Changes.

• During heating (temperature

change) use Q = mct

• During phase changes use heat of fusion or heat of vaporization.

• Q = mLf or Q = mLv

• L = latent heat (unique)

Heating curve of water

• Starting with ice at -4 º C and going to steam at 120 ºC.

Adding energy

ice

liquid

steam

0 º C

100 º C

-4 º C

120 º C

Types of Heat Transfer

• Thermal Conduction-requires objects to touch in order to transfer heat.

• Convection-requires the motion of a fluid between objects in order to transfer heat.

• Radiation-energy moves in the form of electromagnetic radiation in order to transfer heat.

Conduction vs insulation

• The ability to conduct heat is a gradient from good conductors such as metals to poor conductors such as ceramics or plastics. Poor conductors are good insulators. An insulator doesn’t actually inhibit conduction, it is just a poor conductor.