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Stoichiometry is a term chemists use to describe calculations that determine the relative quantities of reactants or products involved in a chemical reaction. Using stoichiometry, chemists can determine the amount of product that can be formed during a chemical reaction from a given amount of reactant. Chemists can also determine the amount of reactant needed to produce a desired amount of product using the same process. Select the missing conversion factor for the following set of calculations. Assume 117 grams of iron(III) oxide, Fe2O3, reacts with excess hydrogen, H2. The problem requires that you determine the mass of iron, Fe, formed from this reaction. Fe2O3 (s) + 3 H2 (g) -> 2 Fe(s) + 3 H2O(l) 117 g Fe2O3 x (1 mol Fe2O3 / 159.70 g Fe2O3) x ______ x (55.85 g Fe / 1 mol Fe) = 81.8 g Fe

          Stoichiometry is a term chemists use to describe calculations that determine the relative quantities of reactants or products involved in a chemical reaction. Using stoichiometry, chemists can determine the amount of product that can be formed during a chemical reaction from a given amount of reactant. Chemists can also determine the amount of reactant needed to produce a desired amount of product using the same process. Select the missing conversion factor for the following set of calculations. Assume 117 grams of iron(III) oxide, Fe2O3, reacts with excess hydrogen, H2. The problem requires that you determine the mass of iron, Fe, formed from this reaction. Fe2O3 (s) + 3 H2 (g) -> 2 Fe(s) + 3 H2O(l) 117 g Fe2O3 x (1 mol Fe2O3 / 159.70 g Fe2O3) x ______ x (55.85 g Fe / 1 mol Fe) = 81.8 g Fe

Stoichiometry is a term chemists use to describe calculations that determine the relative quantities of reactants or products involved in a chemical reaction. Using stoichiometry, chemists can determine the amount of product that can be formed during a chemical reaction from a given amount of reactant. Chemists can also determine the amount of reactant needed to produce a desired amount of product using the same process. Select the missing conversion factor for the following set of calculations. Assume 117 grams of iron(III) oxide, Fe2O3, reacts with excess hydrogen, H2. The problem requires that you determine the mass of iron, Fe, formed from this reaction. Fe2O3 (s) + 3 H2 (g) -> 2 Fe(s) + 3 H2O(l) 117 g Fe2O3 x (1 mol Fe2O3 / 159.70 g Fe2O3) x x (55.85 g Fe / 1 mol Fe) = 81.8 g Fe

Added by Jacob R.

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