Chapter 3- Thermodynamics

Question 1

First Law of Thermodynamics

Answer 1

Energy cannot be created or destroyed

Question 2

Second Law of Thermodynamics

Answer 2

• The entropy of the universe increases
• The universe always tends toward increasing disorder or randomness

Question 3

Enthalpy

Answer 3

Heat content of the reacting system
- Delta H= q

Question 4

When heat energy is absorbed from the environment

Answer 4

Delta H> 0 = Endothermic reaction

Question 5

When heat energy is released to the environment

Answer 5

Delta H< 0= exothermic reaction

Question 6

The entropy of organized/ ordered systems is

Answer 6

Low ( Delta S > 0 when entropy increases)

Question 7

Spontaneous

Answer 7

occurs without work

Question 8

Non-spontaneous

Answer 8

brought about only by doing work (No natural tendency to occur)

Question 9

Gibbs Free energy

Answer 9

Delta G = Delta H - T (Delta S)

Question 10

Delta G < 0

Answer 10

Spontaneous/ exergonic

Question 11

Delta G > 0

Answer 11

Non Spontaneous/ endergonic

Question 12

Delta G= 0

Answer 12

Rxn at equilibrium

Question 13

The more negative Delta G:

Answer 13

The more work the system can do

Question 14

If Keq < 1

Answer 14

Reactants are favored

Question 15

Keq > 1

Answer 15

Products are favored

Question 16

Delta G ^o

Answer 16

-RTln(Keq)

Question 17

The criterion of spontaneity of a reaction is the value of

Answer 17

Delta G

Question 18

Bond energies indicate

Answer 18

how stable a compound is or how easy it is to break a particular bond

Question 19

A larger bond energy means

Answer 19

it is harder to break and the compound is more stable

Question 20

Does breaking a bond release energy?

Answer 20

NO

Question 21

Can heat drive an isothermal chemical process?

Answer 21

NO

Question 22

Net release of Free energy is when the

Answer 22

weakest bonds are broken in favor of the stronger bonds being formed

Question 23

ATP’s energy results from products having a lower

Answer 23

free energy which makes the reactants more stable

Question 24

How can endergonic biochemical reactions run against their thermodynamic potential?

Answer 24

coupling them to highly exergonic reactions

Question 25

when combining multiple reactions, you combine the Delta G ^o values by

Answer 25

adding them

Question 26

When combining multiple reactions, you combine the Keq values by

Answer 26

multiplying them

Question 27

The hydrophobic effect is

Answer 27

an entropic effect

Question 28

a decrease in entropy results in Delta S being

Answer 28

Negative