Chemistry Final Problem Set Cheat Sheet
Notes
- Finding AMU
- C12 = 98.9
- C14 = 1.1
- Empirical -> Molecular
- Find mols of each compound for hydrates or each atom. Divide by lowest.
- Then find empirical
- Combustion Analysis
- of and >> of and of
- //This is stoichiometry, times the mass to find mass of product.
- //The limiting reactant was so we used that to find the mols of
- Variables
- //Avogadro's Number
- Percent Yield
- Statements
- AMU is equivalent to g/mol
- Limiting reactant is x
- Mass Percent
- Abundance
- Gas Law
- Converting Pressure
- Molar Volume
-
- Concentration = number of moles/volume
- Concentrations
-
- Concentration
- Number of Moles
- Volume
-
- Concentration
- Number of Moles
- Molarity = mol/L
- Dilution
- Density
- % Mass >> Molar Concentration
- Examples
- Problem Set - Quantities
- Nitrogen has the following isotopic abundances:
- 14.003074 amu 99.6320%
- 15.000109 amu 0.3680%
- Determine the molar mass of nitrogen
- A compound contains only carbon, hydrogen, and sulphur. A combustion analyzer collects 11.0 g of CO2, 11.26 g of H2O, and 16.0 g of SO2.
- Determine the empirical formula of the compound.
- If the molar mass is 98.0 g/mol, determine the molecular formula.
-
-
-
- = Empirical formula
- A 20.0 g sample of MgSO4 . xH2O is dried yielding 13.78 g of anhydrous salt. Determine the formula of the hydrate.
-
-
- 10.00 g of copper were mixed with 40.00 g of silver nitrate according to the following reaction:
- How much silver was produced?
- Silver nitrate is the limiting reactant