SL Soichiometry
Moles (mol)
using large groups allows us to work with measurable masses when we convert moles to mass.
Avogadro's constant = 6.02 x 10^23 particles (in one mol)
Molar mass
mass of 6.02 x 10^23 particles of a substance. g/mol. Using moles allows us to measure amounts of substances regardless of atom size. you are measuring quanitity.
Empirical Formula
The formula of a chemical compound in its simplest form.
Conservation of Matter
Matter cannot be created nor destroyed
Atom Economy
Evaluates the conservation of natural resources for synthetic and industrial processes. The higher the percentage, the better (the less waste produced).
%AE = (molar mass of atoms of desired product / molar mass of reactants) x100
Atom Economy: Green chemistry
sustainable design of chemical products and chemical processes. aims to minimize the use and generation of chemicals that are hazardous to human health and the environment.
n=
m/M
c=
n/V
concentration
mol OR g dm^-3
Volume
dm^3
molar concentration=
c/M (this is basically either g dm^-3 OR mol dm^-3)
Diluting a solution equation
C1V1=C2V2
Dilution Factor=
10/100 = 10x less concentrated.
ex.
solution 1=0.01 mol dm^-3
solution 2=0.001 mol dm^-3
and so on...
Spectrophotometry
measurement of the intensity of radiation used to determine the concentration of coloured solutions. A spectrophotometer produces light at certain wavelengths which passes through small sample of solution, and a photodetector measures the light intensity that is transmitted and converts it to absorbance.
KNOW THE GRAPH!!
Acid + base =
salt + H2O
Gas Laws STP
P = 100kPa
T = 273K
Vm = 22.7dm^3 mol^-1
n (gas)=
V/Vm
Vm
dm^3 mol^-1
Ideal Gas Laws
1. spaces between particles are bigger than the particles
2. no intermolecular forces except when they collide
3. kinetic energy is proportional to temperature
4. no energy lost when collisions happen
Pressure increases when
volume decreases and temperature increases
Boyles Law
P1V1 = P2V2 (T is constant). Pressure increases, volume decreases
P and V units
pascals and m^3 (or dm^3)
T units
always in K.
K= degrees in C + 273
Charles Law
T1V2=T2V1 (temp increases volume increases)
Gay-Lusacs Law
T1P2=T2P1 (temp increases, pressure increases)
combined gas law equation
(P1V1)/T1 = (P2V2)/T2
R
8.31 dm^3 *kPa K^-1 mol^-1
Ideal Gas Law equation is
PV = nRT
Real Gases two points
1. the volume of the gas particles are not negligible: real gases travel shorter distances and collide more frequently (more pressure)
2. there are no attractive forces between particles: slower speed and less pressure