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Chemistry > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

Gas volume changes with

A

pressure and volume

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2
Q

pressure =

A

force/area

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3
Q

atmospheric pressure decreases with

A

altitude

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4
Q

the 4 variables that determine behavior of gasses

A

pressure, temperature,volume,amount

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5
Q

ideal gas

A

gas that has linear relationships among the 4 variables

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6
Q

are there true ideal gases?

A

no

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7
Q

what is Boyles law?

not the formula

A

at a constant temperature, the volume is inversely proportional to the pressure

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8
Q

what is the formula for Boyles law?

A

PV= constant (p1t1=p2v2)

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9
Q

at fixed pressure and temperature, P decreases as V

A

increases

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10
Q

at a fixed temp. and pressure, P increases as V

A

decreases

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11
Q

What relationship does Boyles law illustrate with gases?

A

pressure & volume

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12
Q

What relationship does Charles law illustrate with gases?

A

temperature and volume

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13
Q

Absolute zero is what?

A

where an ideal gas would have 0 volume

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14
Q

what is the degree for absolute 0?

A

0 Kelvin

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15
Q

What is the proportional part of gases in Charles law?

A

temperature and volume

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16
Q

Volume decreases as temperature

A

increases

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17
Q

volume increases as temperature

A

decreases

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18
Q

what is a unit for force

A

newton

19
Q

what is a unit for area

A

meters^2

20
Q

what is the formula for charles law?

A

v/t = constant (v1t1 = v2t2)

21
Q

what is a unit for pressure

A

pascal

22
Q

What is the combined gas law?

A

P1V1/T1 = P2V2/T2

23
Q

what is STP

A

standard temperature & pressure

24
Q

What is standard molar volume (not the number)

A

volume of 1 mol of an ideal gas at STP

25
Q

What is the value of standard molar volume

A

22.4 L

26
Q

What is the ideal gas law formula?

A

pV=nRT

27
Q

what is the value of R in the ideal gas law formula?

A

0.0821

28
Q

what is the density of a gas INVERSELY proportional to?

A

temperature

29
Q

what is the density of a gas DIRECTLY proportional to?

A

molar mass

30
Q

M and m represent what?

A

M = moles/molarity & m = mass

31
Q

what is the equation for finding density of a gas at STP?

A

d = MxP/RT then convert to moles

32
Q

how do you manipulate the above equation (d=MP/RT) for a change in temperature?

A

add the temperature given to the constant temp. (273 K)

33
Q

what is the equation for finding molar mass from the ideal gas law?

A

M = mRT/PV

34
Q

Gases mix ____________ in any proportions

A

homogeneously

35
Q

the pressure exerted by each gas in a mixture is called its _________?

A

partial pressure

36
Q

what does Daltons law state about gases and pressure?

A

the total pressure is the sum of all of the partial pressures

37
Q

the partial pressure of a gas is proportional to its_____?

A

mole fraction

38
Q

what are the equations for finding total pressure? (Daltons Law)

A 
P(a) = X(a) x P(total)
X(a) = n(a)/n(total)
39
Q

what is the Kinetic molecular theory a model for?

A

Gas Behavior

40
Q

How many postulates (points) are there in the Kinetic molecular theory?

A

three

41
Q

what is the first postulate in the kinetic molecular theory?

A
  • Gas particles are tiny with a lot of space between them

- the volume of each particle is so small compared to the overall volume it is assumed to be 0

42
Q

what is the second point in the Kinetic molecular theory

A

particles are in straight, random, and constant motion except for when they collide with each other or container walls

43
Q

what is the third point in the kinetic molecular theory?

A
  • collisions are elastic (particles transfer energy but do not lose any b/c friction)
  • total kinetic energy is constant
  • particles do not influence each other outside of collisions
44
Q

at a given temperature, all gases in a sample have the same what?

A

average kinetic energy

Chemistry (4 decks)

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