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Flashcards in Module 12 Deck (20)
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1

State Charlie's Law

under conditions of constant pressure, the temperature and volume are linearly proportional to each other
TEMP AND VOLUME PROPORTIONAL

2

Define boiling point

the temperature at which the liquid's vapor pressure is equal to atmospheric pressure.
VAPOR PRESSURE EQUAL TO ATMOSPHERIC PRESSURE

3

pressure

the force per unit area exerted on an object P= F/A

4

Pascal (Pa)

the pressure unit of Newtons/ square m

5

1.000 atm =

101.3 kPa
760.0 torr
760.0 mmHg

6

Boyle's Law

as long as the temperature of a gas stays the same, the product of the gas' volume and its pressure is always the same PV= constant
GAS VOLUME AND PRESSURE IS SAME WITH A CONSTANT TEMP

7

Absolute temp scale

kelvin temp scale that can never reach 0 degrees

8

Extrapolation

following an established trend in the data even though there is no data available for that region

9

combined gas law

PV/ T = constant (p- pressure, v-volume, t- temp)

10

When using any equation in this module, I must always use

the Kelvin Temp scale

11

Ideal gas

a gas that applies to the combination gas law

12

three properties of an ideal gas

molecules/atoms that make it up are very small compared to the total volume available to the gas
MOLECULES SMALL COMPARED TO TOTAL VOLUME

molecules/atoms that make it up are so far apart from one another that there is no attraction or repulsion between them
MOLECULES WITH NO ATTRACTION/REPULSION

the collisions that occur between the gas molecules/atoms must be ELASTIC COLLISIONS

13

elastic in terms of this module

when molecules/ atoms collide with each other or the walls of the container, no energy is lost

14

Standard temp and Pressure (STP)

a temp of 273 K and a pressure of 1.00 atm
used as a reference to determine whether or not a gas is ideal

15

A gas with a temp that is ... and a pressure that is... will behave in an ideal fashion.

close to (or larger than) 273 K
near (or lower than) 1.00 atm

16

Daltons law of Partial Pressures

when ideal gases are mixed, the total pressure of the mixture is equal to the sum of the pressures of each individual gas Pt = P1 + P2 + P3 + …

(Pt= total pressure) (P1, P2 etc are referred to as PARTIAL PRESSURES)

17

The pressure of an ideal gas does not depend on the ... It depends only on the...

identity of the gas
quantity of that gas

18

vapor pressure

the pressure exerted by the vapor which sits on top of any liquid

19

the vapor pressure of any liquid ...

increases with increasing temp

20

mole fraction

X = # of moles of component/ total # of moles in the mixture