Unit 6

Question 1

System

Answer 1

the place that the experiment is held

Question 2

surroundings

Answer 2

everything that surrounds the system

Question 3

open system

Answer 3

energy and matter is transfered from surroundings

Question 4

closed system

Answer 4

only energy is transferred from the surroundings

Question 5

isolated system

Answer 5

nothing is transferred from the surroundings

Question 6

State Function

Answer 6

a measurement of thermodynamics that only depends on the initial and final states, nothing in between matters

Question 7

extensive properties

Answer 7

properties at non standard states

Question 8

intensive properties

Answer 8

properties at standard states, signified by naught

Question 9

standard state

Answer 9

1 atm
1 mol/whatever stochiometric coeff

Question 10

exo -

Answer 10

negative value

Question 11

endo -

Answer 11

positive value

Question 12

Kinetic Energy (KE) equation

Answer 12

1/2 (mass)(volume)^2 = (kg) x (m/s)^2 = Joules

Question 13

Potential Energy (PE)

Answer 13

stored energy

Question 14

Potential Energy equation

Answer 14

K(qq / r ) = (constant) [(charges) / (distance)]

Question 15

Energy equation

Answer 15

E = PE + KE

Question 16

First Law of Thermodynamics
Law of Conservation

Answer 16

Energy cannot be created or destroyed

Question 17

How do we measure Energy?

Answer 17

heat

Question 18

Specific heat

Answer 18

Raising one gram of a substance by one C

Question 19

1 calorie is…

Answer 19

4.184 Joules

Question 20

heat equation (q)

Answer 20

q = mcΔT

m = mass in grams
c = specific heat
T = temp change in Kelvin or C

Question 21

What is the unit of heat?

Answer 21

JOULES

Question 22

Equation of Delta E

Answer 22

q + w
= (heat) + (work)

q + PΔV

Question 23

Hess’s Law

Answer 23

Operation performed on equation is performed on the heat of the reaction

Question 24

Formation Reaction

Answer 24

Where reactants are made from their basic elements from their purest form
1 mol
1 atm

Question 25

Heat of Formation

Answer 25

the amount of heat needed for a formation reaction

Question 26

ΔH (naught) equation for a reaction

Answer 26

Σ(ΔH of formation of products) - Σ(ΔH of formation of reactants) OR ΔH ≈ Σ(bond energies of reactants) - Σ(bond energies of products).

Question 27

specific heat capacity vs molar heat capacity

Answer 27

one gram vs one mol

Question 28

If work is done ON the system, the sign is...

Answer 28

+

Question 29

If work is done BY the system, the sign is...

Answer 29

-

Question 30

Enthalpy

Answer 30

Heat produced or absorbed by a reaction

Question 31

Delta H/Enthalpy change equation

Answer 31

(H products) - (H reactants)

Question 32

Bomb Calorimeter

Answer 32

Constant Volume

Question 33

Bomb Calorimeter Equation of Delta E

Answer 33

ΔE = q_v

Question 34

Pressure constant Calorimeter

Answer 34

ΔE = ΔH - PΔV

Question 35

Energy needed to break bonds are always...

Answer 35

positive

Question 36

What does Gibbs Free Energy Measure?

Answer 36

Determining the amount of energy available from any chem reaction, which determines spontaneity

Question 37

Gibbs Free Energy Equation

Answer 37

ΔG = ΔH - TΔS OR ΔG _0 (products) - ΔG _0(reactants)

Question 38

What type of reactants are spontateous?

Answer 38

NEGATIVE G value

Question 39

ΔG _0

Answer 39

At standard temp

Question 40

ΔG _0 and ΔG relationship

Answer 40

ΔG = ΔG° + RTlnQ

Question 41

When is Q = K, and what does K tell us?

Answer 41

at equilibrium k > 1 = products are favored, spontaneous k < 1 = reactants are favored, nonspontaneous

Question 42

Entropy (S)

Answer 42

The number of disorders in a system

Question 43

higher particles mean... (entropy wise)

Answer 43

higher entropy

Question 44

higher volume mean.. (entropy wise)

Answer 44

higher entropy

Question 45

change of state (!) mean... (entropy wise)

Answer 45

higher entropy

Question 46

above all, more gaseous particles mean...

Answer 46

higher entropy

Question 47

Entropy for elements are...

Answer 47

NOT zero, like delta H and delta G

Question 48

Boltzmann Equation - Entropy

Answer 48

S = k ln W k = constant W = microstates

Question 49

Delta S naught

Answer 49

ΔS° = Σ (ν * S°(products)) - Σ (ν * S°(reactants))

Question 50

Entropy in a reversable process

Answer 50

S = q rev / T = ( heat added) / (T) = J / K