Moles Flashcards
(29 cards)
1dm3 - cm3
X1000
1m3 - dm3
X1000
1cm3 - mm3
X1,000,000
1g - mg
X1000
1kg - g
X1000
1 tonne - kg
X1000
What is the definition of a mole?
The amount of substance that has the same number of particles as there are carbon atoms in exactly 12g of carbon 12.
What is the mass of one mole of a substance called?
Molar mass
Same as atomic number
What are the units of molar mass?
grams per mol
What are the 3 ways to find the moles?
mass/molar mass
volume/molar volume
concentration X volume
What is the molar volume?
24dm3 OR
24000cm3
What are the units of volume?
dm3
What are the units of concentration?
moldm-3
How do you work out the number of particles?
Moles X Avogadro’s constant
What is Avogadro’s constant?
6.02 X 10^23
How do you prepare a standard solution?
Place beaker on scales. Zero it.
Add 0.59g of salt into the beaker using spatular.
Add distilled water, stir with glass rod until salt has dissolved.
Add solution to volumetric flask using funnel.
Slowly add distilled water until bottom of meniscus is at 100cm3.
Put bung in and invert 15 times to mix.
What is the empirical formula?
Simplest ratio of atoms of each element present in a compound
How do you work out the empirical formula?
Work out number of moles of each element
Divide each by smallest one
What is the molecular formula?
Number and type of atoms of each element in a molecule.
How do you work out the number of water molecules in water of crystallisation calculations?
Moles of water/
Moles of anhydrous salt
What is the ideal gas equation
pV=nRT
What is pressure measured in the ideal gas equation?
Pascals
Pa
What is volume measured in the ideal gas equation?
m3
What is temperature measured in the ideal gas equation?
Kelvin
K
