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Chemistry 2016-2017 > Gas Laws > Flashcards

Gas Laws Flashcards

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1
Q

What did Boyle discover

A

Pressure-volume relationship

For a given mass of a gas at a constant temperature, the volume of a gas varies inversely with pressure

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2
Q

What did Charles discover

A

Temperature and volume of a gas at constant pressure
For a given mass of a gas at a constant pressure, the volume of the gas is directly proportional to its temperature in Kelvin

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3
Q

What did Gay-Lussac discover

A

Temperature and pressure
For a given volume of gas, as the temperature of an enclosed gas increases, the pressure of a gas is directly proportional

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4
Q

Combined gas law

A

Relationship between temperature, pressure, and volume of a gas

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5
Q

True or false: Boyle’s law states that pressure is inversely proportional to volume

A

True

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6
Q

True or false: Charle’s law states that volume and temperature are directly proportional

A

True

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7
Q

True or false: Gay-Lussac’s law states that pressure and temperature are directly proportional

A

True

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8
Q

True or false: If the pressure is increased by a factor of 3 times then the volume will increase by a factor of 2 times

A

False

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9
Q

True or false: If the temperature is increased by a factor of 2 times then the pressure will increase by a factor of 2 times

A

True

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10
Q

True or false: Decreasing the volume of a container by 1/2 will double the pressure

A

True

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11
Q

True or false: A graph of volume vs. temperature will produce a curve

A

False

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12
Q

True or false: A graph of an inversely proportional relationship will produce a straight line

A

False

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13
Q

True or false: When steam condenses in a closed container a partial vacuum is created

A

True

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14
Q

True or false: A balloon placed in cold water will increase in volume

A

False

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15
Q

Kinetic Theory of Matter

A

All particles of matter are in constant motion

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16
Q

How does the Kinetic Theory of Matter work for solids

A

Particles are moving so so so slowly it is practically impossible to see

17
Q

Gases are made up of

A

Tiny particles of negligible volume (very very small)

18
Q

Random walk definition

A

Gas particles move in a straight line until they hit something and then change direction

19
Q

All collisions between gas particles are

A

Elastic

20
Q

Elastic definition

A

The gas particles do not stick together when they collide

21
Q

Can KE be transferred?

A

Yes but it cannot be lost

22
Q

As the number of collisions increase

A

Pressure increases

23
Q

How will the collisions increase

A

More particles

Increase in temperature causes more frequent collisions of gas particles with other gas particles and walls

24
Q

Name of a space with no gas pressure

A

Vacuum

25
Q

Definition of ideal gases

A

Gases that follow all rules of the kinetic molecular theory

26
Q

What did Dalton discover

A

Gas pressure depends on the amount of gas and the average kinetic energy of its particles
Total pressure of a mixture of gases is = to the sum of its individual partial pressures

27
Q

What did Graham discover

A

Diffusion and effusion

The rate of effusion of a gas is inversely proportional to the square root of the the gas’ molar mass

28
Q

Diffusion definition

A

The tendency of gas particles to spontaneously spread out until uniformly distributed

29
Q

Effusion definition

A

The escape of a gas through a tiny pinhole in a container of gas

30
Q

An ideal gas has

A

No molecular volume, no attractive forces

31
Q

In reality are ideal gases real

A

There are no perfectly ideal gases but under most conditions, real gases will mostly act like ideal gases

32
Q

When do gases not act like ideal gases

A

High pressure, low temperature, high molar mass, and polar molecules

Chemistry 2016-2017 (11 decks)

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