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Please know the topic of Molar Mass/Conversions before attempting stoichiometry.
Simple Explanation:
Stoichiometry uses mole ratios to study the quantitative relationships between the reactants and products of reactions.
It allows us to predict the:
Amount of reactants required for a reaction.
Amount of products that can be formed from a reaction.
Stoichiometry is based on the Law of Conservation, which means that matter cannot be created or destroyed during a reaction.
Key Concepts
Mole Ratios: The ratio of the amounts (in moles) of each substance involved in a balanced chemical reaction,
Information about ratios originates from the coefficients in the balanced chemical equation.
Example: In this reaction: 2H₂ + O₂ → 2H₂O, 2 moles of H₂ and 1 mole of O₂ are needed to make 2 moles of H₂O.
Excess Reactants: What reactants we have an excess amount of.
Limiting Reactants: What reactants run out first in a reaction.
Percent Yield: Measures efficiency of a reaction.
(Actual Yield ÷ Theoretical Yield) × 100
Simple Demonstration of Concept:
Solve for moles of substance B if 3 moles of substance A were to react with an excess amount of substance B.
Chemical Equation: A + 2B → 2C
For every 1 mole of substance A, 2 moles of substance B are required to react with it. Therefore, if 3 moles of substance A are reacted, the amount of substance B needed must be double that of substance A. This means 6 moles of substance B are required, assuming an excess of substance B is available.
Introduction Video:
Solution Stoichiometry:
TO BE ADDED
Gas Stoichiometry:
TO BE ADDED
Enthalpy Stoichiometry:
TO BE ADDED
Electrolysis Stoichiometry:
TO BE ADDED
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