2C The mole Flashcards
Mole
The amount of substance containing as many elementary particles as there are carbon atoms in 12g of the isotope Carbon-12
Avogadro’s constant
6.02 x 10^23
Molar mass
The mass per mole of substance.
Moles equation (Using Mr)
moles = mass ÷ Mr
Mass equation
Mass = Moles x Mr
Mr equation
Mr = Mass ÷ moles
Empirical formula
The simplest whole number ratio of atoms of each element present in a compound
Molecular formula
The actual number. ratio and type of atoms of each element present in a molecule.
Water of crystallisation
Water molecules that are bonded into a crystaline structure of a compund
Anhydrous
Salt without water
Hydrated
Salt with water
When reacting masses use:
Equation. Moles off known. Moles off unknown. Answer
Solute
A solid which can dissolve in a solvent
Solvent
A liquid which can dissolve a solute
Solution
A solvent with a solute dissolved in it
Concentration
The amount of solute, in moles, dissolved per 1 dm^3 of solution
Standard solution
A solution of known concentration
Concentration equation
Concentration = Moles ÷ Volume (dm^3)
Moles equation (using concentration)
Moles = concentration x volume
Volume equation
Volume = Moles ÷ concentration
1 dm^3 in cm^3
1000cm^3
Molar gas volume at rtp
24dm^3
Moles equation (using gas volumes)
Volume of gas ÷ 24
Volume of gas
Moles x 24
what does a smaller volume to do pressure
increase in pressure
what does a smaller temperature to do pressure
Decrease in pressure
what does more moles of gas do to pressure
increase in pressure
What is the ideal gas equation?
PV=nRT
How many pascals in 1 atm
10^5 Pa
How many pascals in 1 Kpa
10^3 Pa
0ºC in kelvin
273ºk (celcius to kelvin = x + 273)
0ºk in celcius
-273ºc (Kelvin to celcius = x -273)
1m^3 in cm^3
10^6 cm^3
1m^3 in dm^3
10^3 dm^3
Percentage error
(Uncertainty ÷ value measure) x 100