Flashcards in Chapter 5 Deck (44):

1

## Gas volume changes with

### pressure and volume

2

## pressure =

### force/area

3

## atmospheric pressure decreases with

### altitude

4

## the 4 variables that determine behavior of gasses

### pressure, temperature,volume,amount

5

## ideal gas

### gas that has linear relationships among the 4 variables

6

## are there true ideal gases?

### no

7

##
what is Boyles law?

(not the formula)

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

8

## what is the formula for Boyles law?

### PV= constant (p1t1=p2v2)

9

## at fixed pressure and temperature, P decreases as V

### increases

10

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

### decreases

11

## What relationship does Boyles law illustrate with gases?

### pressure & volume

12

## What relationship does Charles law illustrate with gases?

### temperature and volume

13

## Absolute zero is what?

### where an ideal gas would have 0 volume

14

## what is the degree for absolute 0?

### 0 Kelvin

15

## What is the proportional part of gases in Charles law?

### temperature and volume

16

## Volume decreases as temperature

### increases

17

## volume increases as temperature

### decreases

18

## what is a unit for force

### newton

19

## what is a unit for area

### meters^2

20

## what is the formula for charles law?

### v/t = constant (v1t1 = v2t2)

21

## what is a unit for pressure

### pascal

22

## What is the combined gas law?

### P1V1/T1 = P2V2/T2

23

## what is STP

### standard temperature & pressure

24

## What is standard molar volume (not the number)

### volume of 1 mol of an ideal gas at STP

25

## What is the value of standard molar volume

### 22.4 L

26

## What is the ideal gas law formula?

### pV=nRT

27

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

### 0.0821

28

## what is the density of a gas INVERSELY proportional to?

### temperature

29

## what is the density of a gas DIRECTLY proportional to?

### molar mass

30

## M and m represent what?

### M = moles/molarity & m = mass

31

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

### d = MxP/RT then convert to moles

32

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

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

33

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

### M = mRT/PV

34

## Gases mix ____________ in any proportions

### homogeneously

35

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

### partial pressure

36

## what does Daltons law state about gases and pressure?

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

37

## the partial pressure of a gas is proportional to its_____?

### mole fraction

38

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

###
P(a) = X(a) x P(total)

X(a) = n(a)/n(total)

39

## what is the Kinetic molecular theory a model for?

### Gas Behavior

40

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

### three

41

## what is the first postulate in the kinetic molecular theory?

###
-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

## what is the second point in the Kinetic molecular theory

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

43

## what is the third point in the kinetic molecular theory?

###
-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