Solution-Performing a mass to mass stoichiometry problem

Performing a mass to mass stoichiometry problem

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When performing a mass to mass stoichiometry problem, explain why masses must be converted to moles rather than directly using the mass of reactants to predict the mass of products. Consider the synthesis reaction of Mg and O2 below. If equal masses of these reactants are allowed to react, explain how you would know which reactant is the limiting reactant and which reactant is the excess reactant. (Lesson 8)

2 Mg + O2 → 2 MgO

Reference no: EM131056977

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Performing a mass to mass stoichiometry problem : When performing a mass to mass stoichiometry problem, explain why masses must be converted to moles rather than directly using the mass of reactants to predict the mass of products.

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Performing a mass to mass stoichiometry problem

Reference no: EM131056977

Reference no: EM131056977

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