3.1.2 Amount of substance Flashcards
Avogadro’s Constant (Nₐ):
6.02 x 10²³
Moles [2]:
- The unit of amount of substance
- One mole is equal to 6.02 x 10²³ particles
Number of moles =
molecular mass (Mᵣ)
Relative atomic mass(Aᵣ) [definition]:
The average mass of an atom compared with 1/12 the mass of an atom
Relative molecular mass(Mᵣ) [definition]:
The average mass of a molecule compared with 12g of a carbon 12 atom
What is the standard reference point in chemistry?
Carbon 12
Avogadro’s Constant [info]:
One mol of any substance contains 6.02 x 10²³identical atoms/molecules/ions of that substance
Moles and concentration:
Number of moles =
Concentration x volume (dm³)
Number of particles =
Avogadro’s constant (Nₐ) x Number of moles
Molecular formula [definition]:
The number of atoms of each element in a molecule
Empirical formula [definition]:
The smallest whole-number ratio of atoms of each element in a compound
The ideal gas equation:
pV=nRT
ideal gas equation meanings [5]:
p= pressure in Pa V= volume in M³ n= mol R= the gas constant (8.31 J K⁻¹ mol⁻¹ t= temperature in K
°C —> K =
+273
Mole [definition]:
The amount of substance that contains the same number of particles as there are in 12g of carbon 12
Standard solution [definition]:
A solution of known concentration
How do you make a standard solution?
-They are made by dissolving an accurately weighed, mass of solid in a volume of solvent using a volumetric flask
Volumetric flask [description]:
It has a thin neck which is marked with a line so it can be filled accurately to its correct capacity
Concentration [definition]:
A measure of how much solute is dissolved per unit solvent
Concentration [equation]:
Concentration = amount of solute (mol)
(mol/dm³) ————————————
. volume of solvent (dm³)
Concentration [equation for cm³]:
Concentration = amount of solute x 1000 (mol)
(mol/dm³) ————————————
. volume of solvent (cm³)
Percentage yield [definition]:
Percentage of how much product was actually made compared with the amount of product that was expected
Percentage yield [equation]:`
Percentage yield = Actual yield
(%) —————————– x 100
. Theoretical yield
Atom economy [definiton]:
The percentage of the total mass of reactants that can be converted into desired product
Atom economy [equation]:
mass of desired product
————————————- x 100
total mass of reactants