quantitative chem 3 Flashcards
percentage mass of an element in a compound =
Ar * number of atoms of that element/
Mr of the compound * 100
moles =
mass / Mr
volume of gas =
mass of gas /
Mr of gas *24
concentration (g/dm cubed) =
mass(g) /
volume (dm cubed)
concentration(mol/dm cubed) =
number of moles(mol) /
volume (dm cubed)
atom economy =
relative formula mass of desired products /
relative formula mass of all reactants *100
percentage yield =
mass of product actually made /
maximum theoretical mass of product *100
Why do you never get 100% yield
Not all reactants react to make a product(reversible)
There might be side reactions
You lose some product when you separate it from the reaction mixture
(yield) what happens if you want to keep the liquid
you lose a bit that remains with the solid and filter paper
(yield) what happens if you want to keep the solid
some of it will get left behind when you scrape it off the paper
what is the atom economy
tells you how much of the mass of the reactant is wasted when manufacturing a chemical and how much ends up as useful product
disadvantages of low atom economy
use up resources quickely make lots of waste product unsustainable aren't profitable raw materials are expensive waste is expensive to remove
the best way of getting rid of waste product
find a use for it
what is concentration
The amount of a substance in a certain volume of a solution
The more solute the more concentrated
why is the a amount of product formed directly proportional to the amount of limiting reactant
if you add more reactant there will be more reactant particles to take part in the reaction.