 # The Arithmetic of Equations

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The Arithmetic of Equations
Section 9.1

Interpreting Chemical Equations
In terms of moles: Example Equation: 2H2 + O2  2H2O 2 mol H2 + 1 mol O2 = 2 mol H2O

Interpreting Chemical Equations
In terms of particles: You know that Avogradro’s Number relates particles and moles (6.02 x 1023 particles = 1 mole) Example Equation: 2H O  2H2O 2 mol H2 x x 1023 particles + 1 mol 1 mol O2 x x 1023 particles = 1 mol 2 mol H2 x x 1023 particles 1 mol 1.204 x 1024 particles of H 6.02 x 1023 particles of O = 1.204 x 1024 particles of H2O

Interpreting Chemical Equations
In terms of mass: 1 mole = molar mass of element or compound Example Equation: 2H O  2H2O 2 mol H2 x grams + 1 mol 1 mol O2 x grams = 1 mol 2 mol H2 x grams 1 mol grams of H grams of O = grams of H2O

Interpreting Chemical Equations
In terms of volume: 1 mole = 22.4 Liters Example Equation: 2H O  2H2O 2 mol H2 x L 1 mol 1 mol O2 x L = 1 mol 2 mol H2 x L 1 mol 44.8 L of H 22.4 L of O = 44.8 L of H2O

After reading Section 9.1, you should know:
How to balance a chemical equation How to calculate particles, moles, volume and mass from a balanced equation