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Reactants in Accordance with the Percent Yield
General Chemistry • Chemical Reactions
Frequently Asked Questions
How do I calculate the required reactant amount when percent yield is less than 100%?
First convert the desired actual product mass to theoretical product mass using m_theor = m_actual / (percent_yield/100). Then convert to moles of product, apply the balanced-coefficient mole ratio to get reactant moles, and convert reactant moles to grams using molar mass.
Why do I need a balanced chemical equation for percent yield stoichiometry?
The balanced coefficients provide the mole ratio between reactants and products. Without a balanced equation, the stoichiometric conversion from product moles to reactant moles is not defined correctly.
What is the difference between actual yield and theoretical yield in this calculator?
Actual yield is the product mass you want to obtain in practice, while theoretical yield is the product mass implied by perfect conversion at 100% yield. The calculator uses percent yield to convert actual yield into the larger theoretical amount needed for stoichiometric sizing.
How should I enter formulas with subscripts and parentheses in the reaction input?
Use standard chemical notation with parentheses and subscripts, such as Ca(OH)2 or Fe2(SO4)3. Separate species with + and separate sides with -> (or →); state labels like (aq) are optional and ignored.