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Finding significant figures for multiplication and division, you must
round your answer to the same number of significant figures as the measurement with the least sig figs
Finding significant figures for addition and subtraction
you must pick and round too the measurement with the least amount of decimal points
Law of Constant Proportions
a chemical substance will maintain its mass in proportions
Molar Mass
The comprising efforts of a compounds atomic weight on a larger scale
(mass)/(molar mass)
moles
moles x molar mass
mass
Mass Spectrometry is used to
calculate the average mass of one element that has multiple isotopes
Emprical formula
The simplest ratioed measurement of the amount of atoms in a chemical formula
Molecular Formula
The actual amount of atoms in elements in a given compound
How too calculate the Empirical Formula
1) convert % of of substance into grams
2) convert grams too moles using molar mass
3) Divide all moles by the smallest value (too ratio out formula)
How too calculate the Molecular Formula
1) calculate EFM
2) molar mass/ molar mass of EFM (each compound)
3) multiply every subscript of the EFM by n (what you multiply)
amu
(mass of isotope) x (relative abundance of isotope) / 100
units for atomic mass
amu
units for molar mass
g/mol
grams → moles
grams x ( 1 mol/ atomic mass)
moles → molecules
moles x (6.022×1023 ) / 1 mol