The Mole, Stoichiometry, and Solutions
Key conversions, formulas, and vocabulary for mole calculations, reaction stoichiometry, and solution concentration.
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Questions Covered in This Set
10 cards to master
What is Avogadro's number and what does it represent?
6.022 × 10²³ — the number of particles (atoms, molecules, ions) in one mole.
What is molar mass and what are its units?
The mass of one mole of a substance, numerically equal to its atomic/molecular mass in amu; units are g/mol.
How do you convert grams to particles?
You must go through moles: divide grams by molar mass to get moles, then multiply by 6.022 × 10²³.
Calculate the molar mass of CO₂.
12.01 + 2(16.00) = 44.01 g/mol
What do the coefficients in a balanced equation represent?
Mole ratios between substances — never mass ratios.
What is the universal stoichiometry 'spine'?
Grams of A → moles of A → (mole ratio) → moles of B → grams of B.
How do you identify the limiting reactant?
Convert each reactant to moles of product; whichever gives the smaller amount of product is limiting, and that amount is the theoretical yield.
What is the formula for percent yield?
% yield = (actual yield ÷ theoretical yield) × 100
Define molarity and give its formula.
Concentration in moles of solute per liter of solution: M = mol solute / L solution.
What equation is used for dilutions, and why does it work?
M₁V₁ = M₂V₂ — because adding water doesn't change the number of moles of solute.
