Thermodynamics 17.1-17.3

Question 1

What is the first law of thermodynamics?

Answer 1

Energy cannot be created or destroyed, however energy can be converted from one form to another

Question 2

System

Answer 2

The molecules involved in the reaction taking place

Question 3

Surroundings

Answer 3

What contains the system

Question 4

When heat is absorbed by the system,

Answer 4

+q ; Endothermic; System is lower than surroundings

Question 5

When heat is given off by the system,

Answer 5

-q; Exothermic; System is higher heat than the surroundings

Question 6

Endothermic is +heat on the

Answer 6

Reactant Side

Question 7

Exothermic is +heat on the

Answer 7

Product Side

Question 8

Spontaneous processes

Answer 8

Precedes without the continual input of energy from an external force

Question 9

Entropy

Answer 9

A measure of the amount of disorder in a system

Question 10

The more disorder in a system, the more

Answer 10

entropy within the system

Question 11

Is entropy a state function like enthalpy?

Answer 11

Yes

Question 12

When energy is dispersed, enthalpy increases/decreases

Answer 12

increases

Question 13

What is the second law of thermodynamics?

Answer 13

Entropy of the universe will increase for a spontaneous process

Question 14

Microstates

Answer 14

Number of different snapshots is needed to describe all possible arrangements of a system

Question 15

As temperature increases, Entropy increases/decreases

Answer 15

Increases

Question 16

As temperature decreases, Entropy increases/decreases

Answer 16

Decreases

Question 17

As volume decreases, Entropy increases/decreases

Answer 17

decreases

Question 18

As pressure decreases, Entropy increases/decreases

Answer 18

Increases

Question 19

Moles on the reactant are greater than the products, Entropy increases/decreases

Answer 19

decreases

Question 20

Moles of the products are greater than the reactants, Entropy increases/decreases

Answer 20

Increases

Question 21

Is the phase change from solids->liquid->gas or is it gas->liquid->solids

Answer 21

solids->liquid->gas

Question 22

Does the entropy increase or decrease:
4Fe(s) + 3O2(g) -> 2Fe2O3 (s)

Answer 22

Decrease; Inaccurate phase change

Question 23

solid to liquid

Answer 23

Melting

Question 24

Liquid to solid

Answer 24

Freezing

Question 25

Liquid to gas

Answer 25

Evaporation

Question 26

Gas to liquid

Answer 26

Condensation

Question 27

Solid to gas

Answer 27

Sublimation

Question 28

Gas to solid

Answer 28

Deposition

Question 29

Gas to gas

Answer 29

No phase change

Question 30

If Enthalpy (H) is exothermic (-) and Entropy (S) is positive (+), the reaction will be

Answer 30

Always spontaneous

Question 30

If Enthalpy (H) is endothermic (+) and Entropy is negative, the reaction will be

Answer 30

Always nonspontaneous

Question 30

If Enthalpy (H) is endothermic (+) and Entropy (S) is (+), the reaction will be

Answer 30

Spontaneous at high temperatures and nonspontaneous at low temperatures

Question 30

If Enthalpy (H) is exothermic (-) and Entropy (S) is negative (-), the reaction will be

Answer 30

Spontaneous at low temperatures and nonspontaneous at high temperatures

Question 30

A given reaction is spontaneous at low temperatures and nonspontaneous at high temperatures. What can be said about enthalpy and entropy?

Answer 30

Enthalpy is - and entropy is -