Amount of Substance Flashcards
Nitrate ion
NO3-
Sulfate ion
SO42-
Carbonate ion
CO32-
Hydrogencarbonate ion
HCO3-
Phosphate ion
PO43-
Nitric acid
HNO3
Sulfuric acid
H2SO4
Ethanoic acid
CH3COOH
Kinetic theory of gases
Most volume is occupies by empty space, particles are far apart.
Constantly moving in random directions, but in straight lines.
Standard states
Temperature - 273K
Pressure - 100KPa
Ideal Gas Equation
pV = nRT
Relative Atomic Mass, Ar
average mass of an atom of an
element
1/12th x the mass of one atom
of carbon-12.
Relative Molecular Mass, Mr
average mass of one molecule of
an element or compound
1/12th x the mass of one atom
of carbon-12.
Relative Formula Mass, Mf
average mass of one formula
unit of a compound
1/12th x the mass of one atom
of carbon-12.
Avogadro’s Constant
6.023x10^23
A mole
One mole contains 6.023x10^23 atoms, ions or molecules.
The mass of a mole of atoms in an element is the Ar of the element.
Finding the number of atoms/molecules/ions
number of moles x Avogadro’s constant
Finding moles of solids
number of moles = mass/Mr
Finding moles in solution
number of moles = concentration x volume.
Atomic number
The number of protons in the nucleus of its atom - it identifies the element.
Mass number
The total number of protons and neutrons in the nucleus.
Isotope
Atoms of the same element with different numbers of neutrons.
Relative Isotopic Mass
Mass of one isotope
1/12 x the mass of a carbon-12
atom
Units (K, m3)
Degrees + 273 = K
cm3 / 1000 = dm3 / 1000 = m3
Percentage Yield
Tells us about the practical efficiency of the process.
Yield = the number of moles/grams of a specified product / theoretical maximum number of moles/grams of the product x 100.
How can yield be lost?
The practical process of obtaining a product.
Reversible reactions do not go to completion.
Heat loss, incomplete combustion.
Atom economy
mass of desired product/total mass of reactants x 100
What is atom economy
Found from the balanced equation of a reaction.
Tells us in theory how many atoms will be wasted.
Empirical Formula
The simplest whole number ratio of atoms of each element in a compound.
Molecular Formula
The actual number of atoms of each element in a compound.
Calculating Empirical Formula
- Divide mass (or % mass) of each element in its compound by its Ar (finding moles).
- Divide each number by the smallest overall mole value.
Empirical Formula with a Hydrated Salt
They have the formula xH2O, where x is the number of water molecules attached to each salt molecule.
What are Back Titrations?
A two-stage analytical technique.
1. Reactant A of an unknown [] is reacted with excess Reactant B of known [].
2. A titration is performed to determine the amount of reactant B.
They are used when: one reactant is volatile, an acid or base is insoluble, a reaction is too slow.