The following question was posed to the physicist Richard Feynman, winner of the Nobel Prize for his work on the theory of quantum electrodynamics: If,

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Presentation transcript:

The following question was posed to the physicist Richard Feynman, winner of the Nobel Prize for his work on the theory of quantum electrodynamics: If, in some cataclysm, all of scientific knowledge were to be destroyed, and only one sentence passed on to the next generation of creatures, what statement would contain the most information in the fewest words?

He said: I believe it is the atomic hypothesis (or the atomic fact, or whatever you wish to call it) that all things are made of atoms - little particles that move around in perpetual motion, attracting each other when they are a little distance apart, but repelling upon being squeezed into one another.

In that one sentence, there is an enormous amount of information about the world, if just a little imagination and thinking are applied.

Temperature and Heat Part 1: Temperature Scales

0 th Law of Thermodynamics If system A is in thermal equilibrium with system B, and system B is in thermal equilibrium with system C, then A and C are in thermal equilibrium (have same temperature)

Thermal Expansion

Volume Thermal Expansion

Temperature and Heat Part 2: Specific Heat and Latent Heat

Specific Heat Capacity

The amount of water that a bucket can hold is called the capacity of the bucket. The more the bucket can hold, the greater its capacity.

The heat capacity of a substance is the amount of heat that 1 kg of it can “hold” before its temperature raises by 1  C. The more heat it takes to raise the temperature, the larger the heat capacity.

How much heat energy (Joules) is required to raise the temperature of this glass of water 1  C? 250 mL (0.25 kg)

It takes 1050 Joules to raise the temperature of this glass of water 1  C. Therefore it takes 4200 J to raise the temperature of 1 kg 1  C. 250 mL (0.25 kg)

The Specific Heat (Heat Capacity) of Different Substances 1  C 2  C 3  C 4  C 5  C I need 448 J/(kg  C) Iron I need 4200 J/(kg  C) Water I need 900 J/(kg  C) Aluminum I need 388 J/(kg  C ) Zinc I need 387 J/(kg  C) Copper I need 377 J/(kg  C ) Brass I need 128 J/(kg  C) Lead

How much heat energy is required to heat 0.5 kg of copper 25  C? (0.5 kg)  (25  C)  (387 J/(kg  C) = 4838 J How much heat energy is required to heat 0.5 kg of water 25  C? (0.5 kg)  (25  C)  (4200 J/(kg  C) = 52,500 J

How much energy is released when 0.5 kg of water cools 25  C? (0.5 kg)  (25  C)  (4200 J/(kg  C) = 52,500 J

Metal A Metal B Metal C Metal DMetal E

Conservation of Energy Heat gained = Heat lost