Chapter 3: Thermodynamics Flashcards

1
Q

Temperature measures these parts of internal energy…

A

Rotational
Transitional
Vibrational

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2
Q

6 Internal Energies

A
  1. ) Vibrational Energy- atoms vibrations within a molecule; atoms in monatomic gas have NO vibrational energy
  2. ) Rotational Energy- molecular movement where spatial orientation of the body changes and center of mass remains fixed; Atoms in a monatomic gas have NO rotational energy
  3. ) Transitional energy- movement of center of mass of a molecule
  4. ) Electronic Energy- potential electrical energy created by attractions b/n electrons and their nuclei; below 5000K, all molecules are at lowest energy level and if no molecular run occurs, electronic energy remains ms constant
  5. ) Intermolecular potential energy- energy created by the intermolecular forces b/n molecular dipoles; gas at room temp & pressure, IPE makes small contribution to internal energy but at higher pressure contributions become more significant
  6. ) Rest Mass energy- energy predicted by e=mc^2
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3
Q

Seven state functions

A

Title. State function. Prefix
1 Internal Energy. U
2 Temperature. T
3 Pressure. P
4 Volume. V
5 Enthalpy. H
6 Entropy. S
7 Gibbs energy. G

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4
Q

Zeroth law of thermodynamics states…

A

That temperature exists

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5
Q

Internal energies (vibrational, transitional, and rotational) describe energies of ….

Sum of these energies is called

Relationship in Increase in thermal energy is

A

Molecular motion

Thermal energy

Increase in temperature

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6
Q

Molecules vibrate faster in a…

Molecules in a solid only…

A

Solid as temps increase

Vibrate

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7
Q

Define enthalpy

A

H=U+PV

Units for Enthalpy is joules (energy)

(U=internal energy)

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8
Q

Change in enthalpy

A

(Delta)H=(delta)U+P(delta)V

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9
Q

Catalysts do not affect…

A

Equilibrium and enthalpy change

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10
Q

Catalyst affect …

A

The rate

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11
Q

What’s Entropy

A

Natures tendency toward “disorder” or the concept of “probability”

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12
Q

Second Law Thermodynamics

A

Entropy of isolated system will never decrease

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13
Q

The sum of entropy is…

A

Change of entropy system + change in surroundings = change in universe > or = 0

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14
Q

Entropy of system can ___________ only if at the same time the surroundings __________ by > or = magnitude

A

Decrease

Increases

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15
Q

Entropy dictates what?

A

Direction of a reaction

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16
Q

Entropy increases with…

A

Number
Volume
Temperature

If a reaction INCREASES the NUMBER of gaseous molecules, then the reaction has (+) entropy

17
Q

Units of entropy

A

J/K

18
Q

Change in entropy process will be the SAME as change in entropy for a _______ process between same 2 states

A

Reversible

19
Q

Entropy is an EXTENSIVELY property which means…

A

It INCREASES with amount of substance

20
Q

Three types of equilibrium

A

Mechanical - when system is NOT accelerating

Material - in material when no net chemical reaction is occurring and there’s no matter transferring within the system

Thermal - when temp is the SAME throughout; can also be in thermal equilibrium with its surroundings, meaning that’s the SAME temp as its surroundings

21
Q

Important MCAT Equation: Gibbs Free Energy (G)

A

(Delta)G=(delta)H-T(delta)S

Refer to system and NOT surrounding

22
Q

(Delta)G=0 which means…

-(delta)G indicates _______ reaction

A

Equilibrium

Spontaneous

23
Q

Examples of non-PV work

A

Contracting muscles
Transmitting nerves
Batteries

24
Q

Gibbs free energy represents the maximum ….

A

Non-PV work available from a reaction

25
Q

Gibbs function [(delta)G, (delta)S, (delta)H] refer to changes in the ….

Gibbs is a function of both…

A

System

Enthalpy and entropy

26
Q

Reaction produces ____ change in enthalpy and a _____ change in entropy, the reaction can NEVER be the spontaneous.

Reaction produces a ____ change in enthalpy and a _____ change in entropy, it must be SPONTANEOUS.

If signs of both enthalpy and entropy are the same for a reaction, then the spontaneity of the reaction will depend on _______.

A

Positive; Negative

Negative; Positive (decreasing; increasing)

Temperature

27
Q

Oth Law

1st Law

2nd Law

3rd Law

A
  • Temp exists and is a state function (2 bodies with the same system are in equilibrium with the SAME system in thermal equilibrium
  • Energy of an isolated system is conserved for any reaction
  • Entropy of the universe INCREASES for any reaction
  • Perfect crystal at 0 K is assigned an entropy value of 0. All other substances and temps have a (+) entropy value
28
Q

Summary:

1) heat and work are the only two ways to change the energy of a _________.
2) heat and work result in the change in ______ energy of a system at REST.
3) Temperature is as _______ and Pressure is as _______.
4) Think of enthalpy as ______, or think of change in enthalpy at CONSTANT pressure as ______.
5) Think of ENTROPY as the __________.
6) Entropy _________ with _______, _________, and __________.
7) Gibbs energy change is as a _____ of maximum amount of energy available to do _______ work such as electrical work in a cell.

A

1) SYSTEM
2) INTERNAL
3) thermal/mole and thermal/vol
4) U+PV; heat
5) SPREADING of energy
6) INCREASES with temperature, volume, and numbers
7) NEGATIVE; nonPV work