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Chem-109 > Test 3 Formulas, units and symbols > Flashcards

Test 3 Formulas, units and symbols Flashcards

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1
Q

Formula: KE avg =

A 
KEavg = 1/2m(Urms)^2
m = mass of the object in kg
Urms = root-mean-square-speed of a gas
KEavg = average Kinetic energy
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2
Q

Formula: Urms =

A 
Urms = sqrt((3RT)/M)
Urms = root-mean-square-speed of a gas
sqrt = square root
R = Universal gas constant
T = Temperature of gas, Kelvin
M = molar mass of the gas, ( kg/mol )
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3
Q

Units: Urms

A

m/s, meters per second

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4
Q

Units: R

A

8.314 J / mol*K

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5
Q

Kinetic molecular theory states

A

at any given temperature, a population of gas particles has the same average kinetic energy

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6
Q

Root-Mean-Square_Speed is

A

The speed of a gas molecule possessing the average kinetic energy

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7
Q

Effusion is the

A

process by which gas molecules escape through a small hole

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8
Q

Formula: Graham’s Law

A

Rate1 / Rate2 = sqrt(M2 / M1)
Rate = Urms
M = molar mass of the gas, ( kg/mol )

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9
Q

Formula: First law of thermodynamics

A 
dEsys = -dEsurr
dE = Change of energy
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10
Q

Formula: dEsys =

A 
dEsys = q + w
q = dHeat
w = work
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11
Q

Formula: w =

A 
w = -PdV
w = work, under conditions of constant pressure
P = pressure
dV = change in volume
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12
Q

-qlost = qgained, is used in

A

Calorimetry

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13
Q

Calorimetry is the

A

science associated with determining the heat transfer during chemical reactions or physical changes

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14
Q

Formula: Heat capacity =

A 
qcal = C*dT
qcal = J
C = Heat capacity, J / degC
dT = Change in temperature
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15
Q

Formula: Molar heat capacity =

A 
qmol = n*Cp*dT
gmol = J
n = number of moles
Cp = molar heat capacity, J / mol * degC
dT = Change in temperature
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16
Q

Formula: specific heat capacity =

A 
qgram = m*S*dT
qgram = J
S = specific heat capacity, J / g*degC
m = mass in grams
dT = Change in temperature
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17
Q

Formula: dH*rxn =

A 
dH*rxn = Sum (dH*fproducts) - Sum (dH*freactants)
dH*rxn = Standard enthalpy change
dH*f = Standard enthalpy of formation
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18
Q

Heat capacity (C)is

A

the amount of energy requried to raise the temperature of an entire object by 1 degC

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19
Q

Molar heat capacity (Cp)

A

the amount of energy required to raise the temperature of 1 mol of a substance by 1 degC at constant pressure

20
Q

Specific heat capacity (s) is

A

the amount of energy required to raise the temperature of 1 gram of a substance by 1 degC at constant pressure

21
Q

Formula: qp =

A 
qp = dH
qp = heat at constant pressure
dH = change of enthalpy
22
Q

Unit: dE =

A

change of energy

23
Q

Unit: dH =

A

change of enthalpy

24
Q

Endothermic reaction

A

heat is absorbed, and the system has a positive symbol

25
Q

Exothermic reaction

A

heat is released, and the system has a negative symbol

26
Q

Open system

A

Mass: exchanges mass with surroundings
Heat: exhanges heat with surroundings

27
Q

Closed system

A

Mass: Does not exchange mass with surroundings
Heat: Exchanges heat with surroundings

28
Q

Isolated system

A

Mass: Does not exhange mass with surroundings
Heat: Does not exchange heat with surroundings

29
Q

Standard heat of formations is also known as

A

The standard enthalpy of formation

30
Q

Standard state rules for a gas

A

the standard state for a gas is the pure gas at a pressure of exactly 1 atm

31
Q

standard state rules for a liquid or solid

A

the standard state for a liquid or solid is the pure substance in its most stable form at a pressure of 1 atm and at the temperature of interest

32
Q

standard state rules for a substance in solution

A

the standard state for a substance in solution is a concentration of exactly 1M

33
Q

Standard enthalpy change, symbol and rule

A

dH*, the change in enthalpy for a process when all reactants and products are in their standard states. The degree sign indicates standard states

34
Q

standard enthalpy of formation, symbol and rules

A

dHf,
pure compound: the change in enthalpy when one mole of the compound forms from its constituent elements in their standard states
Pure element in its standard state: dHf = 0

35
Q

Written summary of the dH*rxn = formula

A

to caldulate dH*rxn, subtract the enthalpies of formation of the reactats multiplied by their stoichiometric coefficients from the enthalpies of formation of the products multiplied by their stoichiometric coefficients

36
Q

Hess’s law

A

if a chamical equation can be expressed as the sum of a series of steps, then dHrxn for the overall equation is the sum of the heats of reactions for each step

37
Q

Relationships involving dHrxn (3)

A
  1. If a chemical equation is multiplied by some factor, then dHrxn is also multiplied by the same factor
  2. if a chemical equation is reversed, then dHrxn changes sign
  3. if a chamical equation can be expressed as the sum of a series of steps, then dHrxn for the overall equation is the sum of the heats of reactions for each step
38
Q

Units and symbol: frequency

A

Hz = 1/s

v

39
Q

units and symbol: wavelength

A

meters

lamduh, (upside down y)

40
Q

Wavelength definition

A

the distance between two analogous points on successive waves

41
Q

amplitude definition

A

vertical measurement from the midline of a wave to the top of a peak or bottom of a trough

42
Q

frequency definition

A

is equal to the number of complete wave cycles that pass through a point in one second

43
Q

The greater the number the frequency the ______ the energy

A

greater

44
Q

the greater the number of the wavelength the ____ the energy

A

lower

45
Q

Frequency and amplitude are directly proportional to the _____

A

energy

46
Q

frequency and wavelength are ______ proportional to the energy

A

inversly

47
Q

order of waves the the electromagnetic spectrum by low energy to high energy

A

radio, microwave, infrared, visible light, ultraviolet, x-ray, gamma ray

Chem-109 (12 decks)

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