Apologia Chemistry Module 2

Front 1

Energy

Back 1

the ability to do work

Front 2

Work

Back 2

the force applied to an object times the distance that the object travels parallel to that force

Front 3

Heat

Back 3

energy that is transferred as a consequence of temperature differences

Front 4

Hypothesis

Back 4

an educated guess explaining observations

Front 5

Theory

Back 5

a hypothesis that has been tested by experiments

Front 6

Scientific law

Back 6

a theory that has been confirmed by many experiments

Front 7

The first Law of Thermodynamics

Back 7

energy cannot be created or destroyed

Front 8

Potential energy

Back 8

energy that is stored

Front 9

Kinetic energy

Back 9

energy that is in motion

Front 10

Joule

Back 10

metric unit for energy that lifts 102g 1 meter

Front 11

Calibration

Back 11

the process of using certain physical measurements to define the scale of a measuring device

Front 12

0.0 C or 32.0 F

Back 12

the temperature of any mixture of ice and water

Front 13

100.0 C or 212.0 F

Back 13

the temperature of any boiling water

Front 14

C = 5/9(F-32)

Back 14

equation for calculating Celsius

Front 15

F = 9/5(C) + 32

Back 15

equation for calculating Fahrenheit

Front 16

Kelvin

Back 16

absolute temperature scale

Front 17

K = C + 273.15

Back 17

equation for calculating Kelvin

Front 18

1 calorie

Back 18

the amount of heat necessary to warm one gram of water one degree Celsius

Front 19

1 calorie = 4.184 Joules

Back 19

relationship between calories and joules

Front 20

1 food calorie (Cal) = 1,000 chemistry calories (cal)

Back 20

relationship between Cal and cal

Front 21

Heat Capacity (or specific heat)

Back 21

the amount of heat necessary to raise the temperature of 1 gram of a substance by 1 degree Celsius

Front 22

Calorimetry

Back 22

the process used to measure heat

Front 23

Experimental scatter

Back 23

The reflection that all measurements have some inacurasies .

Front 24

Heating curve

Back 24

A graph showing how a substance's phases (gas, liquid or solid) changes while being heated.

Front 25

Heat capacity formula

Back 25

q = mc∆T

Front 26

Delta T formula

Back 26

∆T = T(final) - T(initial)

Front 27

Heat capacity units

Back 27

J/g°C or cal/g°C or cal/kg°C

Front 28

Specific heat of water

Back 28

1.000 cal/g°C or 4.184 J/g°C

Front 29

Calibrate a thermometer

Back 29

Note the reading at the temp of ice/water mixture and apply the difference between the reading and the actual tempreture of freezing to future measurements.

Front 30

Calorimetry equation

Back 30

-q(object) = q(water) + q(calorimeter)