Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

MCAT Chemistry > Thermochemistry > Flashcards

Thermochemistry Flashcards

1
Q

First law of thermodynamics

A

Change in internal energy (delta U) = Heat (Q) - Work (W)

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

Adiabatic process

A

No heat exchange

Delta U = -W

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

Isothermic process

A

Constant temperature

Delta U = 0 –> Q = W

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

Isobaric process

A

Constant pressure

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

Isochoric process

A

Constant volume

Delta U = Q

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

What are two process functions?

A

Heat (Q) and work (W)

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

1 cal = ? J

A

4200 J

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

When is enthalpy (delta H) = Q?

A

At constant pressure

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

Heat absorbed or released in a given process = ?

A

q = m.c.delta T

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

What is the specific heat of water?

A

1

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

Heat capacity = ?

A

m.c

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

Equation when using a bomb calorimeter?

A

q sample + q oxygen = (-) q surroundings (water)

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

Equation to use to find equilibrium temperature of two objects?

A

q hot = (-) q cold

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

Heat of phase change = ?

A

q = m. L (latent heat)

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

What is held constant in a bomb calorimeter?

A

Volume

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

What is held constant in a coffee-cup calorimeter?

A

Pressure

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

Enthalpy (Delta H) = ?
(-) ?
(+) ?

A

Heat transferred into or out of the system
(-) : exothermic
(+) : endothermic

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

What is the standard enthalpy of formation, DeltaHf?

A

Enthalpy required to produce one mole of a compound from its elements in their standard states.

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

What is the standard heat of a reaction equal to?

A

Delta Hrxn = Sum of Delta Hf products - Sum of Delta Hf reactants

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

What is Hess’ law?

A

Delta H = Delta H1 + Delta H2 + Delta H3 …

It works for all other state functions as well.

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

What is the bond dissociation energy?

A

Average energy required to break a particular type of bond between atoms in the gas phase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Equation for Gibbs free energy? Mnemonic with the fish!!

A

Delta G = Delta H - T. Delta S

Goldfish are horrible without tartare sauce

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is an exergonic reaction? What is Delta G?

A

Spontaneous: Delta G (-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is an endergonic reaction? What is Delta G?

A

Nonspontaneous: Delta G (+)

25
When is Delta G temperature dependent?
When Delta S and Delta H have the same sign
26
What is the standard gibbs free energy?
Delta Grxn = Sum of Delta G products - Sum of Delta G reactants
27
How to calculate the standard Delta Grxn from Keq?
Standard Delta G rxn = - RT ln. Keq
28
How to calculate the Delta Grxn from Keq and Q? How to estimate the sign of Delta Grxn?
Delta G rxn = RT ln (Q/Keq) = Delta G (standard) + RT.lnQ If Q/Keq
29
What happens to the volume of a substance as it goes from solid to liquid? Why? What is the exception to this rule?
It increases because it becomes less dense Water
30
How can the entropy change in a reaction be estimated? 2 factors
1. number of moles of reactants and products: a. decrease in moles = decrease in entropy b. increase in moles = increase in entropy 2. phase changes a. gas to solid = decrease in entropy b. solid to liquid = increase in entropy
31
Are explosions spontaneous or nonspontaneous?
Spontaneous
32
What is the enthalpy of formation of an element?
Always 0
33
Which side of an exothermic reaction is favored at high temperatures?
Shift to the left!
34
How to apply Hess' law to heats of combustion and heats of formation?
Heat of combustion = sum of the heat of formation of the products - heat of formation of the reactants
35
What is the heat of formation of O2?
0
36
What does the standard heat of formation represent?
The heat necessary to synthesize elements in their standard state
37
What unit to use for all of these equations?
Kelvin!
38
When asked which conditions are favorable to a certain reactions, what are the 2 things you should check?
Moles of gas | Exo or endothermic?
39
What is the equation to calculate entropy?
Delta S = Qrev / T ``` Qrev = heat gained or lost in a reversible reaction T = temperature ```
40
When energy is added to a system, does its entropy increase or decrease?
Increase
41
When energy is removed from a system, does its entropy increase or decrease?
Decrease
42
How to calculate the change in entropy of a system?
Add up the change in entropy of the different elements in the system
43
What is the work of a calorimeter equal to?
0
44
What is the effect on entropy when particles move from high concentration to low concentration?
Increase in entropy
45
If Delta G is (-), then what does this mean for Q?
Q is smaller than Keq
46
What does a negative change in entropy mean?
It decreases
47
Solvation layer formation effects on entropy? Free energy?
Entropy: decrease | Free energy is > 0 --> non spontaneous
48
What is favorable: increasing or decreasing entropy?
Increasing
49
When adding hydrophilic molecules to water, is entropy increased or decreased? How is free energy affected?
Increased | Free energy spontaneous
50
What is the Delta G of passive transport?
(-)
51
What is the Delta G of active transport?
(+)
52
What is Delta G standard ' ?
Standardized for neutral pH = 7
53
What is the pH for standard Delta G?
0
54
How can I use the first law of thermodynamics in the cellular environment?
Fixed volume and pressure, so Delta U = Q
55
What is the equation for the entropy of the universe? What does it mean?
Delta Suniv = Delta S system + Delta S surroundings > 0 Which means: the entropy of a system and its surroundings will NEVER decrease, it will always remain 0 or increase At constant P and T, the entropy of a system will spontaneously increase
56
What does it mean in radioactive decay if there is no tissue damage?
There was no gamma emission
57
When does "all" of a sample is considered to have decayed?
7-8 half lives
58
Which nuclear decay can be detected on an atomic absorption spectrum?
Gamma radiation

MCAT Chemistry (17 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions