Final Exam (not including exams 1-3) Flashcards

1
Q

energy

A

capacity to do work

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2
Q

heat

A

transfer of energy from higher temerpature to lower temperature

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3
Q

thermodynamics

A

study of heat and energy flow during change and the relationship between heat and work

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4
Q

thermochemistry

A

study of heat involved in chemical and physical changes
or
study of heat change in chemical rxns

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5
Q

explosion energy (examples)

A

light, heat, sound, gas, expansion (work)

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6
Q

What does each particle in a system have?

A

kinetic and potential energy

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7
Q

internal energy (E)

A

kinetic + potential energy

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8
Q

joule

A

amount of energy needed to lift a 1 kg mass by 1 meter

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9
Q

calorie

A

amount of energy needed to raise 1 gram of water by 1 degree celcius

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10
Q

system

A

part of the universe that is of interest in the study
* can be anything
* ex. a person, a room

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11
Q

universe

A

system+surroundings

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12
Q

what can be exchanged in an open, closed, and isolated system

A

open: mass and energy
closed: energy
isolated: nothing

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13
Q

kinetic and potential energy are ___

A

inconvertable (not able to be changed)

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14
Q

law of conservation of energy

A

energy cannot be created or destroyed; it is constant

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15
Q

state functions

A

properties that are determined by the current state of the system, regardless of the path taken to reach that state
ex. energy, pressure, volume, temperature
analogy: 2 hikers took different paths but ended up at the same spot

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16
Q

first law of thermodynamics

A

energy can be converted from one form to another but cannot be created or destroyed

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17
Q

heat in an exothermic rxn

A

heat goes from (lost from the) system to surroundings

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18
Q

what are the 2 ways energy is lost from a system

A
  1. converted to heat, q
  2. used to do work, w
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19
Q

work

A

energy transferred when something is moved by a force acting over a distance

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20
Q

when gases expand, change in volume is ___, but the system is doing work on the surrounding, so work is ___

A

positive
negative

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21
Q

exothermic process

A

heat goes from system to surroundings

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22
Q

endothermic

A

heat goes from surroundings to system

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23
Q

standard enthalpy of formation of any element in its most stable form is ____ degrees celcius

A

0

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24
Q

hess’s law

A

the enthalpy change for an overall process is the sym of the enthalpy changes for the individual steps

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25
kinetics
how fast will the rxn proceed
26
how does spontaneity have to do with speed
nothing
27
spontaneous change
occurs without a continuous input of energy from outside the system * leads to an increase in entropy
28
nonspontaneous change
occurs if the surroundings continuously supply energy to the system
29
if a change is spontaneous in one direction, it will be ____
nonspontaneous in the reverse direction
30
spontaneous process
occurs under a specific set of conditions
31
nonspontaneous process
does not occur under a specific set of conditions
32
entropy (S)
measure of how spread out or how dispersed the system's energy is * increases when volume is larger
33
4 processes that lead to an increase in entropy
* melting * vaporization * temp. increase * greater number of gas molecules
34
does entropy increase or decrease with temperature
increases
35
higher entropy when...
* molecules are more complex * molecules are larger * more energy * higher temp * solid to liquid to gas
36
which has a higher entropy: dissolved solid or liquid vs pure substance
dissolved
37
which has a higher entropy: gas dissolved in solution and solid vs pure gas
pure gas
38
entropy (S) is a measure of how ___
dispersed energy is throughout the system
39
2nd law of thermodynamics
no process is 100 efficient heat lost to surroundings
40
standard free energy of rxn
free energy (G) change for a rxn wehn it occurs under standard-state conditions
41
standard state conditions
temp = 298 K pressure = 1 atm [solute] = 1.0 M [H+] = 1 M
42
what does change in free energy tell us
spontaneity and the maximum energy available to do work
43
delta G
change in free energy when pure reactants convert COMPLETELY to pure products
44
what is the keq for product favored rxns
keq>1
45
conditions for reactant favored
change G under standard conditions>0 and K<1
46
oxidation
loss of electrons
47
reduction
gain of electrons
48
oxidizing agent
thing that is reduced
49
reduction agent
thing that is oxidized
50
oxidation number
charge the atom would have in a molecule or compound if electrons were completly transferred
51
anode
the electrode at which oxidation occurs
52
cathode
the electrode at which reduction occurs
53
does the anode or cathode produce the electrons
anode
54
salt bridge
spectator counter ions flow through the salt bridge to keep net neutral charge in the solutions
55
anode is always on the left or right
left
56
conditions for standard reduction potential (E naught)
1 M and 1 atm
57
E naught
sign changes when half-cell rxn is reversed but the number does not change even when coefficients do
58
diagonal rule
species on left with react spontaneously w/ species on the right of any rxn located below it
59
diagonal rule in my own words and applied to the problem
an element on the left side and above the other element is the one that gets reduced; the other element gets oxidized so we flip its equation and the E naught sign
60
when to use subscripts vs coefficients from balance equation
subscripts - breaking a moelcule into its individual element coefficients - moles of reactant or product into moles of another
61
diatomic molecules molar mass
just one - when it's apart of a compound two - when it is alone
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