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Amount of substance (chem0
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Cards (82)
What are the two types of formulae mentioned in the study material?
Empirical
and
molecular formula
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What does the empirical formula represent?
The simplest whole-number ratio of
atoms
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What is the molecular formula of water?
H₂O
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Why is the empirical formula important for non-molecular substances?
It represents the ratio of atoms in
giant structures
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What is relative molecular mass compared to?
The mass of an atom of
carbon-12
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How do you calculate relative molecular mass?
Add
relative atomic masses
of elements
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What is the molar mass of carbon, C?
12.0 g mol⁻¹
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What does the equation n* = *m / *M* represent?
The relationship between
amount
, mass, and
molar mass
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If you have 96.0 g of carbon, how many moles do you have?
8.0 mol
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How do you calculate the mass of 0.050 mol of NO₂?
Multiply
moles
by
molar mass
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What is the molar mass of Na₂CO₃?
106.0 g mol⁻¹
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What is the Avogadro constant?
6.02 ×
10²³
mol⁻¹
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How is the mass of one mole of an element related to its relative atomic mass?
It equals the relative atomic mass in
grams
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How do you convert cm³ to dm³?
Divide by
1000
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What is a standard solution?
A solution of known
concentration
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How do you calculate the amount of Na₂CO₃ needed for a standard solution?
Use
n* =
*c × *
V
* / 1000
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What are the steps to calculate the mass required for a standard solution?
Calculate
moles needed
: n* = *c × *
V
* / 1000
Determine
molar mass
of solute
Calculate mass: m* = *n × *
M
*
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What is the relationship between moles, concentration, and volume in solutions?
Amount of substance
*n* (mol)
Concentration *c* (
mol dm⁻³
)
Volume *V* (
dm³
)
Formula
: n* = *c × *V*
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What are the common volume measurements used in chemistry?
cm³
(
millilitres
)
dm³
(litres)
1 dm³ =
1000
cm³
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How does the mole relate to counting particles?
1 mole =
6.02 × 10²³
particles
Avogadro constant
: *N* = 6.02 × 10²³ mol⁻¹
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What is the significance of the mass of 1 mole of carbon-12?
12 g of carbon-12 contains
6.02 × 10²³
atoms
Links atomic mass to macroscopic measurements
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What is the importance of using the correct formula when working with moles?
Ensures clarity in calculations
Avoids confusion between different
substances
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What is the concentration of the NaCl solution mentioned?
0.160 mol dm⁻³
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How do you calculate the volume of a solution?
Use the
formula
V* = *n × 1000 / *c*
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What is the volume of the solution containing 3.25 × 10⁻³ mol of NaCl?
20.3
cm³
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What is a standard solution?
A solution of known
concentration
Often labeled as 1
mol dm⁻³
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How is a standard solution prepared?
By dissolving an
exact mass
of
solute
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How do you calculate the mass required for a standard solution?
Use the
mole concept
to find mass
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How many moles of Na₂CO₃ are needed for 100 cm³ of a 0.250 mol dm⁻³ solution?
0.0250
mol
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What is the molar mass of Na₂CO₃?
106.0 g mol⁻¹
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How do you calculate the mass of Na₂CO₃ required?
Use
m*
= *
n
× *
M
*
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What is the mass of Na₂CO₃ required for the standard solution?
2.65 g
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How can concentrations be expressed besides mol dm⁻³?
Concentrations can be expressed in
g dm⁻³
Mass concentration
is calculated from
moles
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What is the molar gas volume at RTP?
24.0
dm³ mol⁻¹
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What is the approximate temperature and pressure at RTP?
20°C
and
101 kPa
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How do you convert between moles and gas volumes?
Use
n*
=
*V
/
*V*m
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How do you calculate moles from gas volume in cm³ at RTP?
n*
= *V /
24 000
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What is the amount of H₂ in 480 cm³ at RTP?
0.0200
mol
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What is the volume of 0.150 mol O₂ at RTP?
3.60
dm³
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What are the assumptions of an ideal gas?
Random motion
Elastic collisions
Negligible size
No
intermolecular forces
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See all 82 cards
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