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Chemistry > Module 6a: Gas Laws > Flashcards

Module 6a: Gas Laws Flashcards

End Test 2

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1
Q

What does Kinetic Theory of Matter tell you?

A

A prediction of how matter should behave

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2
Q

T/F: All matter is made up of moving particles

A

T

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3
Q

Solids have tightly bound particles that ______

A

vibrate

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4
Q

Describe the particles in liquids

A

Free to move
still attracted to each other

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5
Q

Describe the particles in gases

A

Far apart
move freely

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6
Q

Phase changes occur with increases in ________ in matter

A

Kinetic energy

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7
Q

What form does kinetic energy normally come in?

A

Heat

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8
Q

What happens when you heat up a solid?

A

Particles can vibrate which increases entropy.
particles break apart and matter liquifies.
Continues to heat up. Can evaporate (turn into gas)

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9
Q

T/F: Physical properties of gases are all similar

A

T

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10
Q

Describe the boiling point of most gases?

A

Low

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11
Q

Gases are composed mainly of __________ elements with ________ formulas, ___________ compounds, and ________ molar masses

A

Nonmetallic
Simple
Small
Low

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12
Q

What are 3 additional characteristics of gasses

A

Expand to fill their container
highly compressible
extremely low densities

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13
Q

What happens when you compress and cool a gas?

A

Turns into a liquid

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14
Q

What type of mixture are 2 gases?

A

Homogeneous mixture

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15
Q

Describe the molecules in gases

A

Move independently
no forces keeping them together or pushing them apart

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16
Q

T/F: Kinetic Theory of Gases: Gases consist of large numbers of molecules that are in continuous, random motion

A

T

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17
Q

T/F: Kinetic Theory of Gases: Attractive and repulsive forces between gas molecules are strong

A

F

weak

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18
Q

When you increase the temperature, the kinetic energy goes ______

A

Up

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19
Q

T/F: Kinetic Theory of Gases: Energy can be transferred between molecules during collisons, but the average kinetic energy of the molecules does not change with time, as long as the temperate of the gas remains constant

A

T

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20
Q

T/F: Kinetic Theory of Gases: Average kinetic energy of gas molecules is dependent on a few factors

A

F

is ONLY dependent on the temperature

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21
Q

_________ is related to the average kinetic energy

A

temperature

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22
Q

u(rms) =

A

The root mean-squared speed

associated with average kinetic speed

23
Q

T/F: At any given temperature, the average kinetic energy of molecules is the same

A

T

24
Q

R =

A

0.08206

25
Q

Temperature is measured in _______

A

Kelvin

26
Q

Describe the relationship between molar mass and particle speed

A

Lower molar mass = higher speed

Higher molar mass = lower speed

27
Q

Kelvin =

A

C + 273.15

28
Q

What does STP mean?

A

Standard Temperature and Pressure

Temp = 273.15 Kelvin

Pressure = 1atm/760mmHg/760torr

29
Q

Pressure Values:

A

1 atm = 760 mmHg = 760 torr

30
Q

Pressure =

A

Force / Area

31
Q

What is Atomospheric Pressure?

A

The weight of air per unit of area

32
Q

What is the atomospheric pressure at sea level?

A

760 mmHg

33
Q

Describe Gas Law: Boyle’s Law

A

P1V1 = P2V2

Pressure inversely related to Volume

Temp is constant

Decrease volume = increase pressure

34
Q

Describe Gas Law: Charles’ Law

A

V1/T1 = V2/T2

Temp directly related to volume

Pressure and amount are constant

increase temp = increase volume

35
Q

Describe Gas Law: Gay-Lussac’s Law

A

P1/T1 = P2/T2

Pressure is directly related to temp

Volume and amount are constant

increase temp = increase pressure

36
Q

What gas law explains why water boils over at a lower temp at higher elevations?

A

Gay-Lussac’s Law

37
Q

Describe Gas Law: Combined Gas Law

A

(P1V1)/T1 = (P2V2)/T2

Combination of Boyle’s, Charles’, and Gay-Lussac’s Law

n is constant

38
Q

Describe Gas Law: Avogadro’s Law

A

V1/n1 = V2/n2

Volume directly related to moles

Temp and pressure are constant

increases moles = increased volume

39
Q

At STP, how much volume does 1 mol of gas occupy?

A

22.4 L

40
Q

n =

A

number of moles

41
Q

Describe Gas Law: Ideal Gas Law

A

PV= nRT

R = 0.08206

42
Q

Describe Gas Law: Dalton’s Law

A

If 2 gases that DO NOT REACT are combined in a container, ACT AS IF THEY ARE ALONE

Pt = P1 + P2 + P3…..

P1 = (n1/nt) x Pt

43
Q

Describe Gas Law: Graham’s Law

A

r1/r2 = sq(M2/M1)

Relates molar mass of 2 gases to their rate of speed

decrease molar mass = increase rate of speed

44
Q

What is effusion?

A

Escape of gas molecules through a tiny hole into an evacuated space until equilibrium is reached.

45
Q

What is diffusion?

A

Spread of a substances through a space from a higher pressure to a lower pressure

46
Q

Describe Gas Law: Henry’s Law

A

Solubility of a gas in a volume of liquid is porportional to partial pressure of that gas in equilibrium with that of the liquid

47
Q

In the real world, the behavior of gases conforms to the ideal gas law only at ______ temperatures and ______ pressures

A

high

low

48
Q

T/F: A gas will show different behaviors at high pressures and low temperatures

A

T

Gases need high temps and low pressures to be predictable

49
Q

T/F: The assumptions of the Kinetic Theory of Gases are tue even when gases are exposed to low temperatures and high pressures

A

F

In the real world, this doesn’t work. This makes gas unstable.

50
Q

Describe Gas Law: Van der Waals Equation

A

Takes into account ideal gas deviations

Adjustments include: Pressure and Volume

(P + N^2 a/V^2) (V-nb) = nRT

HE SAIDDDDDD HE WONT PUT THIS ON THE TEST

51
Q

If we are to ASSUME a volume, what is it?

A

100ml

52
Q

What is w/v?

A

(weight in grams) / 100ml !!!!!!!!!!!!!!!!!

53
Q

What is w/w?

A

(weight in grams) / 100g !!!!!!!!!!!!!!!!!!!!!!!!!!!

Chemistry (13 decks)

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