Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Anatomy and Physiology > Chem Chp 7 > Flashcards

Chem Chp 7 Flashcards

1
Q

Thermodynamics

A

study of energy, work, and heat

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

3 Laws Thermodynamics

A
  1. Energy cannot be created or destroyed only converted from one form to another
  2. Universe spontaneously tends toward increasing disorder or randomness.
  3. Disorder of a pure perfect crystal at absolute zero is zero
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

molecules and atoms are in constant random motion and

A

frequently collide with each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

average kinetic energy of the atoms or molecules ____ with increasing temperature

A

increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Collisions with sufficient enrgy will

A

break bonds in molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

when reactant bonds are broken

A

new bonds may be formed and products result

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

We can only measure change in energy

A

TRUE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

System

A

process under study

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

surroundings

A

encompasses the rest of the universe

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Heat

A

transfer of thermal energy to the surroundings

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

exothermic reaction

A

releases energy to the surroundings

energy to break bonds is less than the energy given off when the bond forms

Energy is product

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

endothermic reaction

A

absorbs energy from the surroundings

energy to break bonds is greater than the energy realeased, the reaction needs more energy

Energy is reactant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Enthalpy

A

Heat

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Change in enthalpy

A

energy released is represented with a negative sign (exothermic)

energy absorbed is shown with a positive sign (endothermic)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Most but not all exothermic reactions

A

are spontaneous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Most but not all endothermic reations

A

are NOT spontaneous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Entropy

A

Measure of the randomness of a chemical system- Represented S

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Reactions that are exothermic and whose products are more disorder will

A

occur spontanously

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Endothermic reactions producting products of low entropy ill

A

not be spontanous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Free Energy

A

Delta G represents the combined contribution of the enthalpy and entropy values

pg 224

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Calorimetry

A

measurement of heat energy changes

22
Q

Calorimeter

A

device used for these measurements

23
Q

Specific Heat

A

The number of calories of heat needed to raise the temperature of 1 gram of the substance 1 degree celsious

24
Q

Heat equation

A

Q= ms x delta T x SH

25
Q

Fuel Value

A

Amount of energy per g of food

26
Q

Nutritional Calorie

A

1 Kilo Calorie (1000 calories)

27
Q

Chemical Kinetics

A

Study of the rate or speed of chemical reactions

28
Q

Only effective collisions have

A

chemical reactions

29
Q

Activation Energy

A

the minimum amount of energy required to initiate a chemical reaction

30
Q

Activated Complex

A

the reaction proceeds from reactatnts to products through an extremely unstable state

31
Q

Formation of the activate complex required

A

energy

32
Q

Because this is an exothermic reaction

A

overall energy change must be a NET realsease of energy

33
Q

Ions in a solution are

A

rapid

34
Q

ractions invlolving covalents

A

generally slower

35
Q

Large Molecules

A

proceed slowly

36
Q

Effective Collisions

A

molecular collisions that have the correct collision oriltation to lead to product formation

37
Q

Rate Increases as

A

Concesntration increases

38
Q

Rate increases as temperature

A

increases

39
Q

Ractions are the fastest in what states?

A

Liquid and Gas

40
Q

Slowest when

A

Solid state

41
Q

Catalyst

A

substance that increases reaction rate

42
Q

Enzymes

A

biological catalyst in body

43
Q

reaction order

A

represents the number of molecules that are involved in the formation of product

44
Q

Complete Reaction

A

one in which all the reactants have been converted to products.

45
Q

Equilibrium reactions

A

no further obvious change is taking place

46
Q

Reversable reaction

A

shown by double arrow

47
Q

Dynamic Equillibrium

A

a situation in which the rate of the forward process is a reversible reaction is exactly balanced by the rate of the reverse process.

48
Q

Equillibrium constant

A

the relationship between the concentration of reactants and products in an equilibrium reaction

49
Q

Le Chatelier’s principle

A

if stress is placed on a system at equilibrium the system will respond by altering the equilibrium composition in such a way as to minimize stress

50
Q

Only gas equilibrium is affected by

A

pressure

51
Q

Catalyst does NOT affect

A

equilibrium

Anatomy and Physiology (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions