- Created by: Pope1912
- Created on: 04-03-15 15:56
A mole is the number of particles.
Amount of substance is measured using a unit called a mole, n.
Molar mass is the mass of one mole and is just the same as relative molecular mass.
Moles = Mass / Mr
Concentration is measured in Mol dm-3.
Number of moles = Concentration x Volume
All gases occupy the same volume when under the same conditions.
Room temperature and pressue = 24 dm3
Number of moles = Volume in dm3 / 24
Ideal Gas Equation
pV = nRT
p = pressure (Pa)
V = volume (m3) 1cm3 = 1 x 10-6 m3 1dm3 = 1 x 10-3 m3
n = number of moles
R = 8.31 J K-1 mol-1
T = temperature (K) K = C + 273
n = pV / RT
Equations and Calculations
Balanced equations have the same number of each atom on both sides.
You can only balance by adding whole compounds.
In ionic equations the charges must balance.
s = solid
l = liquid
g = gas
aq = aqueous (solution in water)
Allow you to find out exactly how much acid is needed to neutralise a quantity of alkali.
Pipette - measure only one volume of solution.
Burette - measure different volumes and allows you to add the solution drop by drop.
Find out what value you need to know.
Number of moles of acid = conc x vol / 100
Conc of alkali = moles of acid x 1000 / vol
Empirical and Molecular Formula
Empirical Formula - gives the smallest whole number ratio of toms in a compound.
n = mass / mols
Divide all by the smallest number of moles.
Molecular Formula - gives the actual numbers of atoms in a molecule.
molecular mass / empirical mass
The theoretical yield is the mass of the product that should be formed in a chemical reaction. It assumes no chemicals are "lost" in the process.
You can use the masses of the reactants and the balanced equation to calculate the theoretical yield.
Number of moles reacted = mass / molar mass
Theoretical yield = moles reacted x molar mass of products
For any reaction the actual mass of the product will always be less than the theoretical yield.
Reasons for this may be: reactants don't react fully, solution gets left on the filter paper, reactants are lost during transfers between containers.
Percentage yield = (actual yield / theoretical yield) x 100
% atom economy = (mass of desired product / total mass of reactants) x 100
Efficiency of a reaction is measured by percentage yield.
Percentage yield does not always represent how wasteful a reaction is.
It may be 100% efficient but most of the atoms end up in by-products rather than the desired product.
Atom economy is a measure of the proportion of reactant atoms that become part of the desired product in the balanced chemical equation.