Day 6: Thermodynamics

Question 1

First law of thermodynamics

Answer 1

Conservation of energy (energy can’t be created or destroyed)

Question 2

Second law of thermodynamics

Answer 2

For spontaneous process, the entropy of the universe increases

Question 3

Third Law of thermodynamics

Answer 3

A perfect crystal at 0K has zero entropy

Question 4

Change in internal energy equation

Answer 4

Δ(E) = q + w
E -> change in internal energy
q -> heat
w –> work

Question 5

Work

Answer 5

w = -PΔV (most common)

Question 6

Gas in a piston: transfer of heat

Answer 6

locks piston

Question 7

Expanding gases

Answer 7

Cool

Question 8

Compressing gases

Answer 8

Warm

Question 9

Isobaric

Answer 9

( ΔP = 0) constant pressure

Question 10

Isochoric

Answer 10

(ΔV = 0) so w=0 Constant volume

Question 11

Isothermal

Answer 11

(ΔT = 0 so ΔE = 0) Constant temperature

Question 12

Adiabatic

Answer 12

(q=0) No heat

Question 13

Expansion

Answer 13

Increase in volume, no work

Question 14

Compression

Answer 14

Decrease in volume, increase work

Question 15

Are heat and work state functions?

Answer 15

No

Question 16

State Functions

Answer 16

independent of pathway (only cares for initial & final states)

Question 17

Entropy (S): phases of matter, from low to high

Answer 17

s

Question 18

Enthalpy (H): Exothermic & Endothermic

Answer 18

Exothermic: (ΔH 0) surroundings get cold

Question 19

Bonded atoms have ________ energy

Answer 19

lower

Question 20

Bonds breaking is

Answer 20

endothermic

Question 21

Bond making is

Answer 21

exothermic

Question 22

ΔH =

Answer 22

∑D(broken) - ∑D(formed)

Question 23

Catabolism

Answer 23

Exothermic

Question 24

Anabolism

Answer 24

Endothermic

Question 25

Enthalpies of formation

Answer 25

ΔH°rxn = Σ ΔH°f (products) - Σ ΔH°f (reactants)

Question 26

Hess’ Law: Formation Reactions:

Answer 26

1. Forms 1 mol of product

2. All elements are in standard state

Question 27

Gibb’s Free Energy (G)

Answer 27

ΔG = ΔH - (TΔS)

Question 28

ΔG

Answer 28

Spontaneous K>1, favors products

Question 29

ΔG>0

Answer 29

Non-spontaneous K

Question 30

ΔG=o

Answer 30

At equlibrium

Question 31

ΔH (-) ΔS (+)

Answer 31

Spontaneous at ALL temperatures

Question 32

ΔH (+) ΔS (-)

Answer 32

Non-spontaneous at ALL temperatures

Question 33

ΔH (-) ΔS (-)

Answer 33

Spontaneous at LOW temperatures (condensation)

Question 34

ΔH (+) ΔS (+)

Answer 34

Spontaneous at HIGH temperatures (Boiling)