Quantitative relationships in chemical reactions.
Stoichiometry applies atomic and molecular conservation to chemical reactions: moles, limiting reactant, excess reagent, conversion, yield and selectivity. Balanced equations give mole ratios; molecular weights convert to mass.
Burning 16 g CH₄ needs 64 g O₂ and gives 44 g CO₂ and 36 g H₂O.
Stoichiometry gives the mass relationships in reactions, so it is the starting point for any process material balance.
Quantitative relationships in chemical reactions.
Stoichiometry gives the mass relationships in reactions, so it is the starting point for any process material balance.
The reactant that is used up first and sets the maximum amount of product that can form.
Reactant supplied in more than the stoichiometric amount, which drives the reaction forward or improves conversion.
Typical applications include calculating the amount of oxygen needed to burn a given mass of methane, finding the yield of a reaction from the limiting reagent and balancing the feed of reactants to match a reaction equation.
Study "Introduction to chemical engineering" first (topic 63 of 100 in Materials & Chemical). It covers the groundwork this topic builds on.
Limiting reactant. Percent yield. Excess air.
Burning 16 g CH₄ needs 64 g O₂ and gives 44 g CO₂ and 36 g H₂O.
The next topic is "Material balances", which builds directly on this one.
It is classed as Intermediate in Materials & Chemical (topic 64 of 100). It is an intermediate topic. Work through the beginner topics in Materials & Chemical first.
Want to practise? Open the interactive course for quick checks, quizzes, simulations and progress tracking.