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IB Chemistry HL > 1 stoichiometric relationships > Flashcards

1 stoichiometric relationships Flashcards

1
Q

homogenous mixture

A

same composition/density throughout.

uniform.

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2
Q

heterogenous mixture

A

different composition/density throughout.

non-uniform

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3
Q

matter can either be

A

pure or a mixture

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4
Q

a pure substance can either be

A

an element or compound

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5
Q

a mixture can either be

A

homogenous or heterogenous

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6
Q

ideally do you want a high or low atom economy

A

high, meaning less waste

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7
Q

atom economy =

A

molecular mass of desired products
————————————————————- x 100
sum of molecular masses of all products

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8
Q

what atom economy would you expect from an addition reaction

A

100%

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9
Q

when is a low atom economy not bad

A

when you have uses for the waste products or can use them in industry

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10
Q

what atom economy would you expect from a substitution reaction

A

less than 100%

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11
Q

what atom economy would you expect from an elimination reaction

A

less than 100%

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12
Q

a high atom economy =

A

fewer waste materials

greener and more economical

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13
Q

percentage yield using moles =

A

moles of product obtained
——————————————- x 100
theoretical moles of product

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14
Q

percentage yield using mass =

A

mass of product obtained
——————————————————- x 100
maximum theoretical mass of product

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15
Q

SI for mass

A

kilograms (kg)

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16
Q

SI for thermodynamic temp

A

kelvin (K)

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17
Q

SI for luminous intensity

A

candela (cd)

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18
Q

masses of atoms are compared on a scale relative to…

A

12C

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19
Q

units of molar mass

A

g/mol

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20
Q

Ar =

A

1/12 mass of one atom of carbon-12

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21
Q

what is an ideal gas

A

one that follows the ideal gas equation and all gas laws.

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22
Q

what are real gases

A

all gases that deviate slightly from gas laws.

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23
Q

what happens to gas particles at a high pressure

A

they get closer together.

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24
Q

what happens to gas particles at low pressure

A

they move less rapidly (less KE) and spread out, leading to greater opportunity for intermolecular forces between the particles to have an effect

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25
what is the ideal gas equation
PV = nRT
26
what is R in the ideal gas equation
8.314
27
what happens to ideal behaviour at low temps and high pressures
it behaves more like a real gas as particles move slower, so intermolecular forces become more significant
28
what happens to a real gas at low pressures and high temperatures
it behaves more like an ideal gas
29
what gases show the most ideal behaviour
those with a low molar mass and weak intermolecular forces between particles
30
what gases deviate from ideal behaviour the most
those with permanently polarized bonds or higher molar masses. this is because there are stronger intermolecular forces between the molecules. if they have strong hydrogen bonds, the deviation is even greater.
31
concentration def
the amount (in mol) or mass (in g) of solute per volume of solution.
32
units of concentration
mol dm-3, | g dm-3
33
concentration =
amount of solute ----------------------------- amount of volume
34
concentration =
amount in moles ------------------------------ volume (dm cubed)
35
ppm is
parts per million
36
what is a primary standard
high purity )99.9%) high molar mass low reactivity does not change composition in contact with air
37
what is serial dilution
diluting a stock solution multiple times usually by the same factor
38
what is volumetric analysis
the precise measurement of volumes to calculate the concentration of a solution.
39
what is a titration
A titration is a method of volumetric analysis in which the concentration of a solution can be determined.
40
the titrant
a burette is filled with a standard solution of known concentration (the titrant)
41
what is analyte
A carefully measured volume of the solution with the unknown concentration (the analyte) is placed in a conical flask below the burette
42
the first trial of a titration is
the rough titration
43
what are concordant values
titration volumes within 0.10cm cubed of eachother
44
what is a back titration
a technique which is useful for analysing impure substances. It is basically a titration done in reverse. In a back titration, an excess of titrant is added to the analyte and the excess titrant is then titrated to determine how much excess titrant remains. Back titrations are commonly used when one of the reactants is insoluble in water but does react with acid, an example being calcium carbonate.
45
what is a standard solution
one of known concentration
46
what is molar concentration
the number of moles of solute dissolved per litre of solution, i.e., M = mol/L
47
moles =
conc x vol
48
1dm cubed =
1000 cm cubed
49
what is R
8.314
50
what should p be in in the ideal gas equation
Pa
51
what should V be in in the ideal gas equation
m cubed
52
what should T be in in the ideal gas equation
kelvin
53
cm cubed to m cubed
divide by 1000000 (10^6)
54
dm cubed to m cubed
divide by 1000
55
celsius to kelvin
+273
56
kpa to pa
divide by 1000
57
absolute zero
0 on kelvin | -273 celsius
58
combination or synthesis reaction
when two or more substances react to produce a single product
59
decompositon reaction
a single reactant being broken down into two or more products
60
single replacement reactions
when one element replaces another in a compound. eg redox
61
double replacement reactions
between ions in a solution to form insoluble substances and weak or non-electrolytes, also termed metatheiss reactions. eg acid base
62
how to get from molecules to moles
divide by avogadros
63
how to get from moles to molecules
multiply by avogadros
64
isotopes
atoms of the same element that have the same number of protons but different numbers of neutrons
65
relative abundance
measure fo how much of each isotope occurs in an element
66
relative atomic mass
Ar | weighted average of the atomic masses of its isotopes and their relative abundances
67
relative molecualr mass/relative formula mass
combining Ar values to form Mr
68
molar mass
mass of one mole of a substance. g/mol
69
qualitative analysis
determining which elements are present in a compound
70
quantative analysis
determining the relative masses of elements
71
how could reduced yield of products be caused
loss of products from reaction vessels impurity of reactants changes in reaction conditions like temp or pressure reverse reactions consuming products in equilibrum systems the existence of side reactions due to the presenve of impurities
72
kinetic theory
most volume occupied by a gas is empty space gaseous particles constantly move in straight lines but random directions gaseous particles undergo elastic collisions with eachother and the container walls. no loss of KE gaseous particles exert no force of attraction on other gases
73
stp vokme
22.7 dm^3 mol^-1
74
boyles law
V1p1 = V2p2
75
charles law
V1 V2 ----- = ------- T1 T2
76
gay-lussac law
p1 p2 ---- = ----- T1 T2
77
combined gas law
p1V1 p2V2 -------- = -------- T1 T2
78
ideal gas equation
pV = nRT
79
why do gases deviate from the ideal gas law at high pressures
molecules have finite volume
80
volume and pressure are....... in a fixed mass of an ideal gas
inversely proportional .
81
is sublimation exo or endothermiv
endothermic
82
is evaporation exo or endothermic
endothermic
83
is condensation exo or endothermic
exothermic
84
avogadro's law
V1 V2 ----- = ------ n1 n2
85
how do you find the limitign reagent
calculate moles and then divide by coefficent
86
1 molecule's mass =
Mr - -------------------- 6. 022 x 10^23
87
for reactions of gases, what cna you use instead of the molar ratio
the volume ratio
88
1 ppm =
1 mg/dm cubed
89
1mg =
0.001 grams
90
pressure =
K ----- V
91
how do you get from atoms to moles
divide by avogadros
92
what is aboslute temperature proportional to
kinetic energy
93
what is Mr/other names
sum of Ar / sum of relative atomic masses relative formula mass relative molecular mass
94
moles to grams
multiply by molar mass
95
grams to moles
divide by molar mass
96
how to calculate molecualr formula
molecular formula Mr -------------------------------------- empirical formula Mr then multiply everythign in the empirical formula by that factor
97
molar conc =
amount of solute ------------------------- volume of solution
98
standard solution is when
the precise conc is known
99
what is avogadros law
equal volumes of gases at the same temp and pressure contain equal numbers of particles
100
which gases show themost ideal behavour
low molar mass | weak intermolecular forces between particles

IB Chemistry HL (12 decks)

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