Amount of substance

Relative atomic mass

The average mass of an atom of an element compared to 1/12 of the mass of an atom of carbon- 12.

Ar

Relative atomic mass

Relative molecular mass

The mass of that molecule compared to 1/12 the relative atomic mass of an atom of carbon-12.

Mr

Relative molecular mass

Mol=

Mass/ Mr

Avogadro constant definition

Number of atoms in 12g of carbon- 12

conc=

mol/vol

Mass standard units

grams (g)

Volume standard units

dm3

cm3 to dm3

divide by 1000

Concentration standard units

mol/dm3

Ideal gas equation

PV=nRT

PV/T=

Constant for a fixed mass of gas

V standard units in ideal gas equation

m3

P standard units in ideal gas equation

Pa

T standard units in ideal gas equation

Kelvin

R standard units in ideal gas equation

JK-1 mol-1

degrees C to Kelvin

add 273

Empirical formula

Simplest whole number ratio of the atoms of each element present in a compound.

% Atom economy=

(mass of desired product/ mass of reactants) x100

Complete combustion makes

CO2 and H2O

Incomplete combustion makes

CO and H2O

Yield=

(product moles/ theoretical max moles of product) x100

kPa to Pa

x1000

cm3 to m3

divide by 1000000