Topic 5 Formulae, Equation & Amounts of substance Flashcards
What is the ideal gas equation?
PV = nRT
P = Pressure (Pa) V = Volume (M^3) n = Amount of gas (Moles) R = Gas constant (8.31 J mol-1 K-1) T = Temperature (Kelvins - Celsius + 273)
What assumptions need to be made when using the ideal gas equation?
- Particles are not attracted to each other.
- Particles have no volume.
What is the equation for moles?
Moles = Mass / Mr
Mass is in grams
What is Avogadro’s constant?
6.02 x 10^23
What does Avogadro’s constant mean?
One mole of a substance is made up of 6.02 x 10^23 of those things. E.g. One mole of bananas is 6.02 x 10^23 bananas / One mole of oxygen is 6.02 x 10^23 atoms of oxygen.
What is a limiting reagent?
A limiting reagent is a reactant in a reaction that dictates how much product is formed.
What is the equation for % yield?
% yield =
Mass of product formed / Maximum theoretical mass
x 100
What is the equation for atom economy?
Atom economy = Mass of wanted product from equation / Total mass of products from equation x 100
What is the equation for concentration?
Concentration = Moles / Volume
or
Concentration = Mass / Volume
Conc = mol dm⁻³ (mol/dm³) Vol = dm³ Mass = g
How do you convert different volumes into m^3?
dm³ / 1000 = m³
cm³ / 1000000 = m³
How do you convert different units of pressure into Pa?
kPa x 1000 = Pa
MPa x 1000000 = Pa
1 atm of pressure = 100kPa
How do you convert degrees Celsius to Kelvins?
Celsius + 273 = Kelvins
How do you calculate back titrations?
Using the ratio of acid:alkali , calculate the moles of alkali that the acid reacts with (should tell you the moles of acid needed to neutralise) in the sample. Then calculate how many moles of alkali react in the resulting solution. Then calculate the final moles of unknown reactant (alkali should be in excess so: amount added - amount reacted = moles of unknown)
What is the definition of empirical formula?
Simplest ratio of each atom in each compound.
What is the definition of molecular formula?
The actual ratio of each atom in each compound.
How do you find the molecular formula from the empirical formula and formula mass?
Empirical formula x
(Formula mass (Mr) / Formula mass of empirical formula)
E.g. Empirical = CH2 Mr = 42 Mr of empirical = 14
42 / 14 = 3
CH2 x 3 = C3H6