Exam 2 Lecture 2 Thermodynamic Flashcards

1
Q

What determines how much internal energy a system has?

A
  • Chemical identity Chemical identity
  • • Sample size
  • • Temperature
  • • Pressure
  • • Physical state (s, l, g)
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2
Q

State function definition

A

• A function or property whose value depends only on the present state of the system, not the path used to arrive at that condition

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3
Q

Examples of state functions

A

– Age – Weight – Location – Elevation

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4
Q

If the system returns to its original conditions, then for a state function of that system…

A

the overall change is zero

Delta state=initial state-final state=0

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5
Q

1

A

C. because you can burn a variable amount of calories depending on the nature of your workout

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6
Q

Explain why location is a state function

A

2

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7
Q

Explain why elevation is a state function

A

3

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8
Q

Internal energy of a nonreacting system is a state function Internal energy of ________

A

a nonreacting system is a state function

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9
Q

The energy change that occurs during a chemical reaction is______

A

Delta E: a state function

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10
Q

What does delta E equal?

A

4

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11
Q

What does q mean 4

A

5 heat

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12
Q

what does w mean 4

A

5 work

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13
Q

Example of electron flow with no conservation of energy

A

6 undamned waterfall (energy converted to sound and heat)

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14
Q

Why is q not a state function?

A

Contributions of q and w can vary depending on how you set the experiment up (pressure or no pressure)

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15
Q

why is w not a state function?

A

Contributions of q and w can vary depending on how you set the experiment up (pressure or no pressure)

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16
Q

Example of electron flow with conservation of energy

A

7 hydroelectric power

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17
Q

Potential energy has proportionate relationships to

18
Q

Kinetic energy has proportionate relationships to

19
Q

Chemical potential energy:

A

stored in bonds

20
Q

– Thermal energy:

A

kinetic energy of molecules

21
Q

– Heat: is ___ energy

22
Q

Work is ___

A

some form of movement

23
Q

——> +energy

A

Delta E = -energy

24
Q

+energy—–>

A

Delta E= +energy

25
\_\_\_\_\_\_\_\_is necessary for work to occur in a chemical reaction
A difference in pressure
26
Describe Delta E in changes in energy and q and w
9
27
Define Enthalpy in terms of p and q
10 In enthalpy, no work is performed
28
If enthalpy is negative
11
29
If enthalpy is positive
11
30
ΔH depends on the _______ of reactants and products
physical states
31
13
14
32
How to determine ΔH experimentally
calorimetry
33
How to determine ΔH experimentally
calorimetry
34
heat Capacity formula
15
35
Specific heat formula
16
36
By \_\_\_\_\_\_\_\_\_\_,\_\_\_\_\_\_\_\_, \_\_\_\_\_\_\_\_, you can determine ΔH for the reaction
the mass of the water, the temperature change, and the specific heat of the surroundings (water)
37
Steps to determine ΔH experimentally
17
38
1 calorie is the same as
the specific heat of water
39
define bomb calorimeter
Volume change is minimized: a device for determining heats of combustion by igniting a sample in a high pressure of oxygen in a sealed vessel and measuring the resulting rise in temperature: used for measuring the calorific value of foods.
40
If no work is performed, then ΔH=
ΔE
41
If there is gas generation or gas consumption, then ΔH doesn't =
ΔE
42
Model why physical state is important to energy used in a reaction