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Chem > Unit 2 > Flashcards

Unit 2 Flashcards

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1
Q

What factors affect gas pressure

A

Gas/number of particles, volume, pressure, temperature

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2
Q

What is a mole

A

6.02x10^23

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3
Q

What is the relation of number of particles and volume

A

Directly related

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4
Q

What is the relationship of temperature and volume

A

Directly related

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5
Q

What is the relationship with pressure and volume

A

Inversely related

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6
Q

What is relation of temp and pressure

A

Directly

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7
Q

Boyles law

A

P1V1=P2V2

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8
Q

Charles law

A

V1/T1=V2/T2

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9
Q

Guy-lussacs law

A

P1/T1=P2/T2

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10
Q

Combined gas law

A

P1V1/T1=P2V2/T2

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11
Q

Avogadros law and STP

A

V1/n1=V2/n2

22.4L/1mole=V2/n2

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12
Q

What is standard temp

A

273K

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13
Q

What is standard pressure

A

1 atm

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14
Q

Molar volume

A

One mile= 22.4L at STP

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15
Q

Dalton law of partial pressure

A

P1+P2+…..Pn=Ptotal

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16
Q

Real gases behave like ideal gases except at

A

Very low temps

17
Q

The gas constant R is equal to .0821 when the pressure is expressed in

A

ATM

18
Q

As more gas particles are added into a container what happens to the collisions

A

Increase because they don’t go as far away from one another

19
Q

What is the relation of proportion for the number of Moles of a gas to its volume at STP

A

Number of moles is directly proportional to its volume

20
Q

Real gases behave like ideal gases expect at —- pressures

A

Low pressures

21
Q

Ideal gas equation will only give correct values if temperature is expressed in

A

Kalvin

22
Q

One mole is how many liters

A

22.4

23
Q

What are different units of pressure

A 
Mm Hg
Atm
Pa
kPa
Torr
24
Q

Elastic collision

A

Using lose velocity when collide

25
Q

Ideal gas

A 
No volume
Elastic collision
Constant straight line random motion 
Don't attract or repel
AVg Kinetic energy directly related to kale in
26
Q

Real gas

A

Volume

Attract each other

27
Q

Gas behavior is most ideal at

A

Low pressures
High temp
Lower attractive force ( non polar)

28
Q

Gases particle motion

A

Random no attraction

29
Q

Gases have low density

A

No volume lots of empty space

30
Q

Diffusion

A

Stays in container but spreads throughout

31
Q

Effusion

A

Leaves container

32
Q

Pressure formula with surface area

A

Force/ SA

33
Q

Density formula

A

D= p(molar mass MM)/RT
D=m/v
P/RT=N/V or m/v

34
Q

Combined gas law with avogadros law

A

PV/nT= R

35
Q

Ideal gas law

A

pV=nRT

36
Q

What causes effusion and deffusion

A

Just molecules moving and mix

37
Q

What causes diffusion to happen slower or faster (rates)

A

Mass

Chem (14 decks)

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