and the concept are key to understanding chemical calculations. They help us quantify substances and their interactions at the atomic level, bridging the gap between the microscopic world of atoms and the macroscopic world we can measure.
These concepts are essential for , which allows us to predict quantities in chemical reactions. By mastering and moles, you'll be able to solve complex chemistry problems and understand how substances interact in precise ratios.
Formula Mass and Mole Concept
Formula masses of chemical compounds
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Formula mass represents sum of atomic masses for all atoms in a chemical formula expressed in () or ()
Calculate formula mass by identifying elements and subscripts in the compound
Locate atomic mass of each element using periodic table
Multiply atomic mass by subscript for each element
Sum products to determine overall formula mass
Example: Calculating formula mass of (C6H12O6)
(): 6 × 12.01 amu = 72.06 amu
(): 12 × 1.01 amu = 12.12 amu
(): 6 × 16.00 amu = 96.00 amu
Formula mass of glucose = 72.06 amu + 12.12 amu + 96.00 amu = 180.18 amu or g/mol
Example: Determining formula mass of ()
(): 1 × 22.99 amu = 22.99 amu
(): 1 × 35.45 amu = 35.45 amu
Formula mass of NaCl = 22.99 amu + 35.45 amu = 58.44 amu or g/mol
Formula mass is used to calculate of compounds
Mole concept and Avogadro's number
represents amount of substance containing same number of particles as atoms in 12 grams of
(6.022×1023) quantifies particles in one mole
One mole of any substance comprises Avogadro's number of particles (atoms, molecules, ions, or formula units)
signifies mass of one mole of a substance numerically equal to formula mass with units of grams per mole (g/mol)
Relationship between moles and Avogadro's number: 1 mole = 6.022×1023 particles and 1 mole of a substance = in grams
Example: One mole of (H2O) contains 6.022×1023 water molecules and has a molar mass of 18.02 g/mol
Example: One mole of sodium (Na) consists of 6.022×1023 sodium atoms and has a molar mass of 22.99 g/mol
Conversions in chemical substances
Conversion factors based on mole concept: 1 mole = molar mass in grams and 1 mole = 6.022×1023 particles
Convert between mass and moles:
Mass to moles: divide mass by molar mass
Moles to mass: multiply number of moles by molar mass
Convert between moles and number of particles:
Moles to particles: multiply number of moles by Avogadro's number
Particles to moles: divide number of particles by Avogadro's number
Convert between mass and number of particles:
Mass to particles: convert mass to moles, then moles to particles
Particles to mass: convert particles to moles, then moles to mass
sets up conversion problems ensuring correct units in final answer
Example: Converting 25.0 grams of water (H2O) to moles
Molar mass of H2O = 18.02 g/mol
25.0gH2O×18.02gH2O1molH2O=1.39molH2O
Example: Determining number of oxygen atoms in 0.500 moles of O2