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chemistryyyy > Unit 3day 4 > Flashcards

Unit 3day 4 Flashcards

1
Q

Write formula for partial pressure of blue

Using ideal gas law

A

Pblue = nblueRT/ V

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2
Q

Formula for total pressure of blue and green

A

Ptotal = Pblue + Pgreen

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3
Q

Write formula for P total

Using ideal gas law

A

P tot= ntotRT/ V

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4
Q

Write formula , for partial pressure of blue gas

Using mol fraction

A

Pblue = mole fraction(X) blue * Ptot

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5
Q

Write formula for mole fraction(X) of blue

Using moles

A

n blue/ n total

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6
Q

Equation for tank valve problems ( one has O2, one has N2)

A

PO2V1 = P’O2Vtot

PN2V2 = P’N2Vtot

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7
Q

Write the formula for total pressure for the tank valve problem

Gases are O2 and N2

A

Ptot= P’O2 + P’N2

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8
Q

Which ballon will have the most efficient reaction? Loudest bang?

A

The one with the most equal mole fraction to molecular formula (empirical)

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9
Q

Ideal gas descriptions

A

TEAR

Tiny- small discrete, far apart
Elastic/Energy - no energy lost or gained
Asexual- not attracted to each other
Random - molecules are constant, random , straight line motion, until they hit a wall

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10
Q

When ranking samples form highest to lowest average KE consider

A

ONLY consider temp

High temp has higher KE

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11
Q

Rank samples from highest to lowest velocity CONSIDER

A

consider both smallest particle(those will be faster) and temp, then use equation if different temp and contradicting different size particles

High temp small particles are faster

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12
Q

Equation for KE of gases with ideal gas law

A

KE = 3/2RT

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13
Q

What does R equal for KE formula with ideal gas law

A

R = 8.314 J/ mol K

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14
Q

Regular formula for KE

A

KE= 1/2m(v^2)

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15
Q

What are the units for the regular KE formulas

A

M (mass) is in Kg
v (velocity) is In m/s(meters per sec)

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16
Q

Which molecule is the lightest for probability density graphs

A

The one that has the flattest most spread out graphs, reaches the highest speed

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17
Q

Which molecule is the heaviest for probability density graphs

A

The molecule that has the highest peak and spreads the least over the x axis, lowest speeds

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18
Q

How does cold molecule graph look

A

Narrow distribution

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19
Q

How does hot molecule graph look

A

Wide distribution

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20
Q

Root mean square velocity , Vrms FORMULA

A

square root of (3RT/mm)

mm in kg/mol

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21
Q

What unit is the mass in for Vrms

Root mean square velocity

A

The molar mass of the element converted to Kg

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22
Q

Diffusion

A

Intermingling of gases due to their random motion

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23
Q

Effusion

A

Escape of gas particles through tiny holes

24
Q

Write mole fraction(X) for blue using pressure

A

Pblue/P total

25
Q

What units does Vrms equation give you

A

M/s

26
Q

What size of particles effuse the best

A

Small particles effuse faster

27
Q

If there’s a solid formed between 2 gases in a tube, where will the precipitate form close to?

A

Next to the gas aight he greater radius because it effuses slower

28
Q

Grahams law

With velocity

A

Va/Vb = sq rt ( mmb/ mma)

29
Q

When to use grahams law with velocity

A

When there’s the same temp and it’s the same molecule you’re comparing

30
Q

Grahams law with temperature

A

Rate a/ rate b = sq rt(Ta/Tb)

31
Q

When to use grahams law with temp(rates)

A

Diff temps same molecule

32
Q

If Z is greater than 1, what are the interactions between gas particles

A

Repulsions

33
Q

If Z is less than 1, what are the interactions between gas particles

A

Attractions

34
Q

How do repulsion’s affect pressure

A

There are more collisions, higher pressure

35
Q

How do attractions affect pressure

A

Less collisions, lower pressure

36
Q

If the experimental pressure is greater than the ideal pressure what does that mean for the interactions between the gas particles

A

Repulsions

37
Q

If the experimental pressure is LESS than the ideal pressure what does that mean for the interactions between the gas particles

A

Attractions

38
Q

Gases behave most ideally at?

A

High temp and low pressure

39
Q

Why do gases behave most ideally at high temp and low pressure

A

A lot of space, so less collisions, and ideally, gases are hot because they come as a result of boiling

40
Q

What rules are not followed for real gases

A

T- Gases are not spaced far apart
A- gases are not asexual because they are not spaced far apart^, they are attracted to each other

41
Q

What does Z equal for an ideal gas

A

1

42
Q

What does Z less than 1, mean for IMFs?

A

High attraction forces if Z < 1 so strong IMFs

43
Q

Hard square Model equation

A

P(V-nb)= nRT

44
Q

What does v equal in hard square model ?

A

Volume of container

45
Q

What does nb equal in hard square model

A

Space occupied by gas

46
Q

Van der Waals Equation

A

(P +a(n^2)/(v^2))(v-nb) =nRT

47
Q

What does a equal in van der waals equation
(Include units)

A

Attractive forces
Atm*L^2/ mol^2

48
Q

What does b equal in hard square model

Include units

A

Size factor

L/mol

49
Q

How do IMFS impact a in van der waals equation

A

Strong IMFS means large a

50
Q

How does size impact b in hard square model

A

Large size(radius) means large b

51
Q

When you think of diffusion think of

A

Mizing

52
Q

When you think of effusion think of

A

Escape

53
Q

The rate of effusion or diffusion equation

A

Va/vb = sq rt(mm a/mm b)

54
Q

What do mol fractions and ONLY mol fractions add to?

A

1

55
Q

What is the unit produced by the standard KE formula

A

Joules

56
Q

What is v in KE = 1/2mv^2

A

Velocity

57
Q

How many mL is 1cm^3

A

1 mL

chemistryyyy (40 decks)

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