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Chem 1 - Amount

Amount of a Substance

Relative Atomic Mass The weighted Average of a mass of an atom of an element, taking into account its naturally occurring isotopes, relative to 1/12th the mass of Carbon-12.
Relative Atomic Mass Formula = Ar = (Average mass of an atom of an element) / (1/12 of mass of atom of Carbon-12)
Relative Molecular Mass The relative molecular mass of a molecule is the mass of that molecule relative the mass of an atom of Carbon-12. Add the Ar of the Atoms in the molecule.
Relative Molecular Mass Formula = Mr = (Average Mass of a Molecule) / (1/12th mass of an atom of Carbon-12).
Avagardo Constant: The Number of molecules in 12 grams of Carbon-12. 6.022 x10^3
Number of Moles = Mass of what you have / Mass of 1 mole (Mr).
Pressure = Force / Area
Describe the effects on pressure for the following variables: Temp, Volume, Number of Moles: Temp: increasing temp increases pressure, the inverse is true. Volume: Increasing Volume decreases pressure, inverse also true. No of Moles, Increasing the no of moles increases pressure, inverse true.
Ideal Gas Constant: PV=nRT (Pressure x Vol = No of Moles x Constant x Temp).
Units of the Ideal Gas Constant Vol = M^3, Temp = Kelvin (K), Pressure = Pa, R = J K-1 Mol-1.
Empirical Formula: A formula showing the simplest whole number ratio of atoms of each element in a compound.
Molecular Formula: A formula showing the actual number of each atom in a compound.
What method is used to find Empirical Formula? Combustion Analysis. Compound is burnt in Oxygen and then the products by mass are analysed.
How to Calculate Empirical Formula: Workout Number of moles of each element, divide all numbers by lowest amount, find ratio.
Moles in a Solution: (Concentration (M) x Volume (V)) / 1000
Concentration = Number of moles / Volume
When can we use the ideal gas equation? To calculate the amount of gas produced in a Reaction
How can we find concentration, experimentally? Using a Titration. So long as we know the concentration of the acid and equation between them.
Write a common Ionic equation: H+ + OH- ---> H20
Titration explain the steps: Fill burette with Acid (known concentration), measure out Alkali with Pipette and add to Flask with indicator, slowly add in acid until neutral, repeat until 2 results are the same.
Atom Economy (percentage): (Mass of desired produce / Amount of reactants) x 100
Reaction Yield (%): (Mass (or moles) of desired product / theoretical maximum amount of desired product) x 100
Created by: mjwilson1988