CHEMISTRY- 3.10 Determining a Chemical Formula
from Experimental Data- STUDY GUIDE WITH
COMPLETE VERIFIED SOLUTIONS
Empirical Formula - ✔✔Represents simplest whole-number ratio of atoms.
Molecular Formula - ✔✔Indicates actual number of atoms in a molecule.
Mass Percent Composition - ✔✔Percentage by mass of each element in a compound.
Molar Mass - ✔✔Mass of one mole of a substance, in g/mol.
Decomposition - ✔✔Chemical reaction breaking down a compound into elements.
Pseudoformula - ✔✔Initial formula using moles as subscripts.
Conversion to Moles - ✔✔Divide mass by molar mass for each element.
Whole-Number Subscripts - ✔✔Final subscripts in empirical formula must be integers.
Step 1: Masses - ✔✔Record masses of each element in the sample.
Step 2: Moles Calculation - ✔✔Convert masses to moles using molar mass.
Step 3: Pseudoformula Creation - ✔✔Write formula using calculated moles as subscripts.
, Step 4: Divide by Smallest - ✔✔Normalize subscripts by dividing by smallest subscript.
Step 5: Whole Numbers - ✔✔Adjust subscripts to whole numbers if necessary.
Example 3.17 - ✔✔Nitrogen and oxygen compound yields empirical formula.
Example 3.18 - ✔✔Aspirin's mass percent leads to empirical formula.
Relative Masses - ✔✔Masses of elements used to determine formulas.
Hydrogen Mass - ✔✔0.857 g of hydrogen from water decomposition.
Oxygen Mass - ✔✔6.86 g of oxygen from water decomposition.
Nitrogen Mass - ✔✔24.5 g of nitrogen from laboratory analysis.
Oxygen Mass (Example) - ✔✔70.0 g of oxygen from nitrogen-oxygen compound.
Carbon Mass (Practice) - ✔✔165 g of carbon from compound decomposition.
Hydrogen Mass (Practice) - ✔✔27.8 g of hydrogen from compound decomposition.
Oxygen Mass (Practice) - ✔✔220.2 g of oxygen from compound decomposition.
Empirical Formula - ✔✔Simplest whole-number ratio of elements in a compound.
from Experimental Data- STUDY GUIDE WITH
COMPLETE VERIFIED SOLUTIONS
Empirical Formula - ✔✔Represents simplest whole-number ratio of atoms.
Molecular Formula - ✔✔Indicates actual number of atoms in a molecule.
Mass Percent Composition - ✔✔Percentage by mass of each element in a compound.
Molar Mass - ✔✔Mass of one mole of a substance, in g/mol.
Decomposition - ✔✔Chemical reaction breaking down a compound into elements.
Pseudoformula - ✔✔Initial formula using moles as subscripts.
Conversion to Moles - ✔✔Divide mass by molar mass for each element.
Whole-Number Subscripts - ✔✔Final subscripts in empirical formula must be integers.
Step 1: Masses - ✔✔Record masses of each element in the sample.
Step 2: Moles Calculation - ✔✔Convert masses to moles using molar mass.
Step 3: Pseudoformula Creation - ✔✔Write formula using calculated moles as subscripts.
, Step 4: Divide by Smallest - ✔✔Normalize subscripts by dividing by smallest subscript.
Step 5: Whole Numbers - ✔✔Adjust subscripts to whole numbers if necessary.
Example 3.17 - ✔✔Nitrogen and oxygen compound yields empirical formula.
Example 3.18 - ✔✔Aspirin's mass percent leads to empirical formula.
Relative Masses - ✔✔Masses of elements used to determine formulas.
Hydrogen Mass - ✔✔0.857 g of hydrogen from water decomposition.
Oxygen Mass - ✔✔6.86 g of oxygen from water decomposition.
Nitrogen Mass - ✔✔24.5 g of nitrogen from laboratory analysis.
Oxygen Mass (Example) - ✔✔70.0 g of oxygen from nitrogen-oxygen compound.
Carbon Mass (Practice) - ✔✔165 g of carbon from compound decomposition.
Hydrogen Mass (Practice) - ✔✔27.8 g of hydrogen from compound decomposition.
Oxygen Mass (Practice) - ✔✔220.2 g of oxygen from compound decomposition.
Empirical Formula - ✔✔Simplest whole-number ratio of elements in a compound.
