Topic 3.2: Thermal Properties of Matter Flashcards

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1
Q

Define specific heat capacity

A

o SPECIFIC HEAT CAPACITY: The amount of thermal energy required to raise the temperature of 1kg of a substance by 1K

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2
Q

Define thermal capacity

A

o THERMAL CAPACITY: The amount of thermal energy required to raise the temperature of an object by 1K.

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3
Q

Define microscopic description

A

o MICROSCOPIC DESCRIPTION: Considers properties of matter at a particle level. Molecules are in motion and collide with each other and the container.

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4
Q

Define kinetic energy of particles

A

o KINETIC ENERGY OF PARTICLES: Temperature is a measure of the average kinetic energy of the particles.

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5
Q

• 3.2.3: Explain the physical difference between the solid, liquid, and gaseous phases in terms of molecular structure and particle motion

A

o PHASES OF MATTER: Particles in a solid are locked into the crystal structure and do not have enough KE to escape. In a liquid, they overcome the chemical bonds but cannot separate completely for the other atoms. The particles in a gas have enough KE to escape from each other.
o Solids –fixed positions, many strong bonds (potential energy)
o Liquids – Changing positions, many temporary bonds
o Gases – Free moving, no bonds

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6
Q

What is the process of going from a gas to a solid?

A

deposition

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7
Q

What is the process of going from a solid to a gas?

A

sublimination

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8
Q

What is the process of going from a solid to a liquid?

A

melting

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9
Q

What is the process of going from a liquid to a solid?

A

solidification

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10
Q

What is the process of going from a liquid to a gas?

A

evaporation

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11
Q

What is the process of going from a gas to a liquid?

A

condensation

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12
Q

• 3.2.6: Distinguish between evaporation and boiling

A

o EVAPORATION: The process by which faster-moving molecules escape from the surface of a liquid. This results in a cooling of the liquid.
o BOILING: The process by which a liquid changes into a solid at the constant temperature of the boiling point.

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13
Q

• 3.2.9: Define pressure and microscopic description of pressure

A

o PRESSURE: The force exerted per unit area. Measured in pascals.
o MICROSCOPIC DESCRIPTION OF PRESSURE: Many moving particles exert forces when they collide with container walls give the effect of pressure being exerted by the gas.

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14
Q

Define ideal gas

A

o IDEAL GAS: A theoretical gas composed of a randomly moving non-interacting particles. It is a useful idea because many real gases behave like an ideal gas unless temperature or pressure are very high or low.

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15
Q

• 3.2.10: State the assumptions of the kinetic model of an ideal gas (6)

A

o KINETIC MODEL OF AN IDEAL GAS: A model which treats a gas as many molecules subject to the following assumptions:
 The molecules obey Newton’s laws
 The intermolecular forces are negligible
 The molecules are spherical with negligible volume
 The motion of the molecules is random.
 The collisions are perfectly elastic.
 The time taken for a collision is negligible.

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16
Q

What is temperature?

A

• 3.2.11: State that temperature is a measure of the average random kinetic energy of the molecules of an ideal gas
o KINETIC ENERGY OF PARTICLES: Temperature is a measure of the average random kinetic energy of the particles.