The Mole Concept and Stoichiometry Flashcards
what is relative atomic mass (Aᵣ)?
average mass of one atom of that element compared to 1/12 of the mass of one carbon-12 atom
*average mass of one atom of an element / 1/12 mass of an atom of carbon-12
what is relative molecular mass (Mᵣ)?
average mass of one molecule of the substance compared to 1/12 of the mass of one carbon-12 atom
*average mass of one molecule of a substance / 1/12 mass of an atom of carbon-12
what is relative formula mass (Mᵣ)?
average mass of one formula unit of the substance compared to 1/12 of the mass of one carbon-12 atom
*average mass of one formula unit of a substance / 1/12 mass of an atom of carbon-12
how do you find percentage mass of an element in a compound?
(Aᵣ x no. of atoms of the element in the formula / Mᵣ of compound) x 100%
what is a mole?
amount of substance that contains the same number of particles as the number of atoms in 12g of carbon-12
*one mole of any substance will always contain 6.02 × 10²³ particles of that substance (Avogadro’s constant/number)
what are the 4 formulae to find the number of moles?
1) n = N / L
- N = no. of particles
- L = Avogadro’s constant (6.02 × 10²³)
2) n = m / Aᵣ or Mᵣ
- m = mass of substance (g)
3) n = v / Vₘ
- v = volume of gas/liquid
- Vₘ = molar volume (24dm³)
4) n = cv
what is the unit for molar mass?
g/mol
*literally the same as Aᵣ/Mᵣ
how do you find the concentration of a solution (g/dm³)?
concentration (mol/dm³) x molar mass (g/mol)
what is stoichiometry?
ratio between the number of moles of reactants and the number of moles of products of the reaction
how do you find percentage yield?
actual yield / theoretical yield x 100%
how do you find percentage purity?
mass of pure element in sample / mass of impure sample x 100%