Thermodynamics Flashcards

1
Q

What is internal energy?

A

The sum of all kinetic and potential energies of all components in the system
DE = E final - E initial
(change in internal energy)

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2
Q

What if the change in internal energy is >0 or <0

A

> 0 = then final is greater than initial. The system has absorbed energy from surroundings - energy change is endergonic

<0 = system released energy to surroundings so energy change is exergonic.

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3
Q

What is the total change in internal energy equal to?

A

Total change in internal energy = q + w
q= heat
w= work

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4
Q

what is endothermic?

A

Heat absorbed by the system from the surroundings - DH is positive

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5
Q

What is exothermic?

A

Het released from system to surroundings - DH is negative

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6
Q

Define internal energy

A

a state function

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7
Q

what is work?

A

When a process occurs in an open container, the only work done is a change in volume of a gas pushing on the surroundings

W = -p DV
p= pressure in Pa
DV - change in volume

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8
Q

what is enthalpy ?

A

if a process takes place at a constant pressure & the only work done is the pressure-volume work, we can account for heat flow during the process by measuring enthalpy change

H = E + PV 
Enthalpy = internal energy + product of pressure and volume
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9
Q

what is DH equal tO?

A

DH = q

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10
Q

Change in enthalpy equation

A

DH = H products - H reactants

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11
Q

How can we measure changes in heat for the system (enthalpy change)?

A

constant pressure calorimetry - aqueous solution, indirectly mesure heat change by measuring what change for water

Bomb calorimetry - measure heat absorbed by water- measure change in internal energy

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12
Q

what is Hess law?

A

if a reaction is carried out in a series of steps, Enthalpy change for the overall reaction will be equal to the sum of the enthalpy changes for the individual steps

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13
Q

Define enthalpy change of formation

A

enthalpy change for reaction in which a compound is made from its constituent elements in their elemental forms
Measured under standard conditions 298K, 1 atm

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14
Q

How is calorimetry used to measure change in enthalpy?

A

Measure heat flow
The change in sample will be felt by the water, heat is transferred to water if it reacts and the thermometer will read it.

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15
Q

Define heat capacity

A

amount of energy required to raise the temperature of a substance by 1K

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16
Q

define specific heat capacity

A

the amount of energy required to raise the temperature of 1g of a substance by 1K

17
Q

Specific heat equation

A

specific heat = heat transferred / mass x temp change

C = q / m x DT

18
Q

What is heat released equal to?

A

Heat released (q) = m x c x DT

19
Q

What is entropy?

A

the disorder in a system
it is a state function
DS = Sfinal - Sinitial

20
Q

What is the change in entropy for a process occurring at a constant temperature

A

DS = q reversible / T

21
Q

Define the second law of thermodynamics

A

Entropy of the universe increases for spontaneous (irreversible) processes, and the entropy of the universe does not change for reversible processes

22
Q

entropy changes for reversible and irreversible processes

A

REVERSIBLE: DS universe = DS system + DS surroundings = no change

IRREVERSIBLE: DS universe = DS system + DS surroundings = increase

23
Q

what law proves that spontaneous processes increase the entropy of the universe?

A

2nd law of thermodynamics

24
Q

How do we calculate entropy on a molecular scale?

A
S = k ln W 
(K = Boltzmann constant) 

Change in entropy is thus:
DS = KlnW final - KlnW initial

25
Q

What are the entropy changes for solids, liquids, gases?

A

S –> L –>G

Gas has the highest entropy - most disorder in system

26
Q

For a process occurring at constant temperature (isothermal) what is the change in entropy of surroundings?

A

DS surroundings = -q system / T
which Is the same as:

DS = DH / T
because q system is DH

27
Q

what is the entropy change of the universe

A

DS universe = DS system + DS surroundings

28
Q

What is the Gibbs free energy equation

A

DG = HD = TDS (at temperatures other than 25 degrees_

29
Q

what happens when DG is negative?

A

It is a spontaneous process. This is because when the universe is positive, DG is negative, and for a spontaneous process, DS universe is always >0

30
Q

How do we find the free energy change (K) from Gibbs free energy?

A

K = e- DG/RT