Chapter 19 - Thermodynamics Flashcards

0
Q

Spontaneous processes

A

Those that can proceed without outside intervention.

Non spontaneous in reverse direction

Temperature matters!

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1
Q

First law of thermodynamics

A

Energy cannot be created or destroyed
Total energy of universe is constant
Can be converted

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2
Q

Reversible process

A

System and surroundings can be put back to original state by exactly reversing the process

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3
Q

Irreversible process

A

Cannot be undone

Spontaneous processes are irreversible

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4
Q

Entropy

A

Measure of randomness
Related to motion in molecules

Change in entropy equals entropy final minus entropy initial

q/t

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5
Q

Isothermal process

A

A process occurring at constant temperature

For entropy the change is equal to heat that would be transferred if reversible divided by temperature

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6
Q

Second law of thermodynamics

A

Entropy of the universe increases for spontaneous processes and does not change for reversible processes

Entropy of universe always increasing

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7
Q

Average kinetic energy

A

Temperature

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8
Q

Motion of molecules

A

Translational: movement of entire molecule from one place to another

Vibrational

Rotational: rotation of molecule about axis or sigma bonds

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9
Q

Microstate

A

Snapshot of molecule notion in a thermodynamic system

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10
Q

Entropy equation with microstates

A

S= k lnW

K is 1.38e-23
W is microstates

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11
Q

Number of microstates increase when

A

Entropy increases
Temperature increases
Volume increases
Molecules increase

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12
Q

Entropy in solutions

A

When solid is dissolves in a solvent, entropy increases

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13
Q

Third law of thermodynamics

A

The entropy of pure crystalline substance at absolute zero is 0

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14
Q

Standard entropies

A

Molar entropy values of substances in their standard state

Tend to increase with increasing molar mass

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15
Q

Size of molecules and entropy

A

Larger and more complex molecules have greater entropies

16
Q

Entropy changes eqn

A

Delta S = sum of m delta S products minus sum of n delta S reactants

17
Q

Gibbs free energy

A

When delta G is negative a process is spontaneous
If positive then spontaneous in reverse direction
If zero it is at equilibrium

18
Q

Free energy changes eqn

A

Delta G = delta H - T * delta S

Enthalpy and entropy terms respectively

19
Q

Under any conditions the free energy change can be found with

A

Delta G = delta G standard + RTlnQ

Rearranged to be

K = e^(-delta G standard/RT)