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General Chem I > Chapter 8 > Flashcards

Chapter 8 Flashcards

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1
Q

What are gases?

A

state of matter where atoms of a substance move

freely and fill their container

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2
Q

What are gases in terms of volume and shape?

A

no fixed volume and shape

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3
Q

What do gases do in containers?

A

uniformly fill them

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4
Q

Are gases easily compressible?

A

yes

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5
Q

How do gases mix with other gases?

A

uniformly mix

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6
Q

What do gases exert for pressure?

A

Exert pressure on their surroundings

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7
Q

What’s the equation for pressure?

A

force / area

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8
Q

What are the units for pressure?

A

atmospheres (atm), mmHg, Torr, Pascal (Pa)

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9
Q

What is atmospheric pressure?

A

is the force exerted on a surface by the air above it due to gravity

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10
Q

What are the variables associated with gases?

A

pressure, temperature, volume, moles

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11
Q

What is STP defined as?

A

standard temperature and pressure as 273.15 K and 1 atm

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12
Q

What is Boyle’s Law?

A

P1V1 = P2V2

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13
Q

What is constant in Boyle’s Law?

A

constant temp

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14
Q

What is Gay-Lussac’s Law?

A

P1/T1 = P2/T2

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15
Q

What is the concept behind Boyle’s Law?

A

When volume decreases,

pressure increases which mean Particles hit the container walls more often

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16
Q

What is the concept behind Gay-Lussac’s Law?

A

When temperature increases,

pressure also increases

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17
Q

What is constant in Gay-Lussac’s Law?

A

constant volume and amount of gas

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18
Q

What is Charle’s Law?

A

V1/T1 = V2/T2

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19
Q

What is the concept behind Charle’s Law?

A

when temperature increases,

volume must also increase

20
Q

What is constant in Charle’s Law?

A

pressure and amount of gas

21
Q

What is Avogadro’s Law?

A

v1/n1 = v2/n2

22
Q

1 mol of ideal gas =

A

22.4 L

23
Q

What is the concept of Avogadro’s Law?

A

Equal volumes of gas contain the same number of particles at the same temperature and pressure

24
Q

To have an ideal gas, what must the motion of the particles be?

A

random

25
Q

To have an ideal gas, what interactions must the gas particles have?

A

no interactions except collisions that are elastic

26
Q

To be an ideal gas, is the identity of the gas relevant or irrelevant?

A

irrelevant

27
Q

To be an ideal gas, what has the be the volume of the gas instead of the gas itself?

A

the volume of the container it occupies

28
Q

What is the Ideal Gas Law?

A

P=nRT

29
Q

In the Ideal Gas Law, what does P equal?

A

pressure

30
Q

In the Ideal Gas Law, what does n equal?

A

moles

31
Q

In the Ideal Gas Law, what does R equal?

A

Gas constant

32
Q

In the Idea Gas Law, what does T equal?

A

temperature

33
Q

What is Dalton’s Law of Partial Pressures?

A

For a mixture of gases in a container, the total pressure

equals the sum of the pressures each gas if it were alone. (p1 + p2 + p3… =p total meaning 2 atm + 7 atm = 9 atm)

34
Q

What is a mole fraction?

A

the ratio of the number of moles of a

a component in a mixture to the total number of moles in the mixture

35
Q

What’s the formula for mole ratio?

A

X1 = n1 / 𝑛𝑇𝑜𝑡𝑎𝑙

= 𝑛1 /𝑛1+𝑛2+𝑛3+…

36
Q

What does the Kinetic Molecular Theory state about volume?

A

Gas particles are so small compared to the distances between them that the volume of the individual particle can be assumed to be negligible or zero

37
Q

What does the Kinetic Molecular Theory state about motion of gas particles?

A

Gas particles are in constant motion

38
Q

What does the Kinetic Molecular Theory state about gas exerting forces on each other?

A

Gas particles are assumed to exert no forces on each other

39
Q

What does the Kinetic Molecular Theory state about the relationship between kinetic energy and the temperature of the gas?

A

they are directionally proportional

40
Q

What does diffusion describe?

A

process of particles moving from an area of high concentration to one of low concentration

41
Q

What does effusion describe?

A

small size enables them to move through small openings as well

42
Q

What does there need to be for effusion to happen?

A

opening of the hole must be smaller than the mean free path because otherwise, the gas could move back and forth through the hole

43
Q

What does Graham’s law of effusion state?

A

The rate of effusion of a gas is inversely related to the square root of the molecular weight of a gas

44
Q

What does Van der Waal’s equation contain?

A

corrected pressure and volume

45
Q

In reality, REAL gases behave more ideal in ___ temperature and ___ pressures

A

In reality, gases behave more ideal in high temperatures and low pressures

46
Q

What is the urms equation for?

A

the measure of the speed of particles in a gas

47
Q

What is Graham’s Law of effusion?

A

R1/R2 = square root of m2 over square root of m1

General Chem I (10 decks)

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