Please enable JavaScript.
Coggle requires JavaScript to display documents.
Module 2: Introduction to Quantiative Chemistry - Coggle Diagram
Module 2: Introduction to Quantiative Chemistry
Law of the Conservation of Mass
Chemical Systems
Open
Closed
Isolated
Stoichiometry
Mole Theory
Mole Ratios
Definition of Moles
6.022x10^23 particles in a substance
Equal to the total atomic mass units (amu) of the substances weighed out in grams
number of moles= mass in grams / molar mass (n=m/MM)
Calculating Yields
Percentage
percentage yield = actual yield/theoretical yield x 100%
Theoretical
Balance Equation
Determine the ratios between reactants and products
Convert the grams of the reactants using n=m/MM, the number of moles in the products can be determined using the molar ratios. The number of grams can be determined using the rearranged formula m= n x MM
Actual
The actual yield (weight in grams)
Concentration
Molarity
number of moles= concentration of moles x volume in litres (n=cV)
Dilution
C1V1=C2V2
Standard Solutions
The mass of the solute needed is calculated and weighed
The solute is dissolved in some distilled water in a beaker
Solution is transferred into a volumetric flask
More distilled water is added to obtain the required volume
The flask is stoppered and shaken
Gas Laws
Gay-Lussac's (other) Law
Pressure and temperature are directly proportional
Avogadro's Law
Pressure and temperature are directly proportional
Gay-Lussac's Law
volume of the gas is related to the number of moles
Boyle's Law
Pressure and volume are inversely proportional
Charle's Law
Volume is directly proportional to temperature
Ideal Gas Laws
the volume (v) occupied by n moles of any gas has a pressure (P) at a temperature (T) in Kelvin (0oC = 273K). PV=nRT, where R is the gas constant (8.314J mol/k)