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Chem
3. Quantitative Chem
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Cards (27)
What is the purpose of quantitative analysis in chemistry?
To determine
formulae
and
reaction equations
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How do analysts use quantitative methods in chemistry?
To determine
purity
and monitor
yield
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Why is classifying chemical reactions important?
It helps
predict
chemical
behavior
and
patterns
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What do chemical equations represent?
Chemical reactions
and communicate ideas
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What does the law of conservation of mass state?
No
atoms
are
lost
or
made
in reactions
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What does a balanced chemical equation ensure?
Equal
numbers of
atoms
on both sides
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What is the relative formula mass (Mr) of a compound?
Sum
of
relative atomic masses
in the formula
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How does the sum of relative formula masses relate in a balanced equation?
Reactants' sum
equals
products' sum
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How can you calculate the percentage by mass in a compound?
Using
relative formula mass
and
atomic masses
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Why might a reaction appear to change mass?
Gas
reactants
or products not accounted for
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What happens when a metal reacts with oxygen?
The
mass
of the
oxide
is greater than metal
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What should students explain regarding mass changes in reactions?
Changes in terms of the
particle model
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What is always present in measurements?
Some
uncertainty
about the result
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How can students represent uncertainty in measurements?
Using the range of measurements about the
mean
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What unit is used to measure chemical amounts?
Moles
, symbol
mol
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How is the mass of one mole of a substance related to its relative formula mass?
They are numerically equal in
grams
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What does one mole of a substance contain?
The same number of
particles
as any mole
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What is the value of the Avogadro constant?
6.02
×
1
0
23
6.02 \times 10^{23}
6.02
×
1
0
23
per mole
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How does the measurement of amounts in moles
apply?
It applies to
atoms
, molecules,
ions
, etc.
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RAM (relative atomic mass)
(mass x abundance)+(mass x abundance)/total abundance
RFM (relative formula mass/Mr)
-add all of the mass numbers together (use
periodic table
)
-include the small numbers
-don't include the large numbers (unless it's atom economy)
No.
moles
mass of sample
(g)/
molar mass
n = m/
Mr
%
atom economy
(total
RFM
desired product
/total RFM
products
) x100
-use big numbers as well when calculating RFM (Mr)
Percentage Yield
(
actual
/
theoretical
) x100
-have to work out
mass
of something to find theoretical yield (
m=nxMr
)
Concentration
c = n/v
(mol/dm^3)
Volume
v = n/c
(cm^3)
mol/dm^3
to
g/dm^3
?
-find the
Mr
of what question asks about (e.g.
sodium carbonate
)
-multiply this by the concentration/volume answer you got in mol/dm^3
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