Physical Chemistry Flashcards

(68 cards)

1
Q

The system can exchange matter and energy with its surroundings

A

Open System

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2
Q

Only energy can be transferred between the system and surroundings

A

Closed system

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3
Q

Neither matter or energy can be exchanged between a system and its surroundings

A

Isolated system

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4
Q

State Function

A

Only the start and the end matter

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5
Q

Path Function

A

It matters how you get there

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6
Q

These are examples of?

  • Internal Energy (U)
  • Enthalpy (H)
  • Entropy (S)
A

State Functions

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7
Q

These are examples of?

  • Heat (q)
  • Work (w)
A

Path Functions

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8
Q

All parts of system within a thermodynamic equilibrium have the same temperature.

A

0th Law

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9
Q

Which law of Thermodynamics covers conservation of energy?

A

1st Law

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10
Q

Which law says state changes will follow the direction of maximum entropy?

A

2nd Law

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11
Q

Which law says that when approaching 0k, entropy becomes constant, so 0 temperature cannot be reached?

A

3rd Law

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12
Q

Charles’ Law

A

An increase in heat creates an increase in volume

Specifically for gas

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13
Q

A gas that doesn’t interact with anything

A

Ideal Gas

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14
Q
A

The state equation of an ideal gas in a closed system

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15
Q
A

Ideal gas law

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16
Q
A

Ideal gas law

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17
Q
A

Avogadro’s law

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18
Q

A transfer of energy that utilizes or causes uniform motion of atoms in the surroundings

A

Work

A force F moving a distance x does work equal to Fx

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19
Q

A measure of the capacity of a system to do work

A

Energy

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20
Q

The means by which energy is transferred from a hotter body to a cooler one in order to equalize their temperatures

A

Heat

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21
Q

The total of the kinetic energy
due to the motion of molecules and
the potential energy

A

Internal Energy

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22
Q

+q: heat is absorbed by the system

A

Endothermic

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23
Q

-q: heat is given out by the system

A

Exothermic

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24
Q

When a gas is compressed by an external
force the work is?

A

Positive

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25
When a gas expands by pushing against an external force the work is?
Negative
26
Energy cannot be created or destroyed but is just transformed from one form to another
1st Law
27
What is the amount of heat needed to raise the temperature of a certain mass 1 degree Celsius?
Heat Capacity
28
Hess's Law
The heat of a whole reaction is equivalent to the sum of its steps
29
When the internal and external pressures are equal the system is in
Equilibrium
30
# Which process * Are infinitely slow * Are at equilibrium * Do maximum work
Reversible
31
# Which process - Go at finite rate - Are not at equilibrium - Do less than the maximum work
Irreversible
32
The process is?
Spontaneous | (irreversible)
33
The process is?
Reversible
34
The process is?
Not possible
35
Gibbs Function
36
The process is?
Spontaneous | (irreversible)
37
The process is?
Equilibrium
38
The process is?
Not possible
39
This is a graphical representation of?
Activation energy
40
Unfolding of regular secondary protein structure causes:
Large increase in the entropy of the protein
41
What does first law of thermodynamics state?
Energy can neither be destroyed nor created
42
Mass does not enter or leave the system in which type of system?
Closed
43
Boiling water represents a ____ in entropy.
increase
44
This has a ___ in entropy?
Decrease
45
The total entropy of the universe ____ in any spontaneous process.
increases
46
The total entropy of the universe ____ in any spontaneous process.
increases
47
Only those processes are possible in nature which would give an entropy ____ for the system and the surroundings together.
increase
48
The disorderly motion of molecules increases and the entropy of the system increases when:
Heat is added
49
# True or False? The heat capacity of the substance is defined as the amount of heat required to raise a unit mass of the substance through a unit rise in temperature.
True
50
Is the formula for?
Enthalpy
51
In a constant volume process, internal energy change is equal to
heat transferred
52
Heat transferred at constant pressure _____ the enthalpy of a system.
increases
53
A reaction is reversible because:
products are reactive
54
If ∆G° of the reaction A → B is -40kJ/mol under standard conditions then the reaction will be:
Spontaneous
55
A large value of Equilibrium Constant Kc means that at equilibrium:
less reactants and more products
56
pKa determines the strength of
an acid
57
In an exothermic reversible reaction increase in temperature shifts the equilibrium to:
reactant side
58
Solubility of Ca(OH)2 is exothermic. Solubility will increase at a ____ temperature.
low
59
The solution having zero pH will be:
highly acidic
60
Decreasing temperature
61
What order reaction is this?
Zeroth
62
What order reaction is this?
First
63
What order reaction is this?
Second
64
Change in the concentration of any one of the reactants or products per unit time is
rate of reaction
65
______ does not affect the rate of a reaction.
ΔH
66
The role of a catalyst is to change the ____________
Activation Energy
67
ΔH < 0
Exothermic
68
ΔH > 0
Endothermic