For each of the following reactions, calculate the grams of...

For each of the following reactions, calculate the grams of indicated product when $15.0 \mathrm{~g}$ of the first reactant and $10.0 \mathrm{~g}$ of the second reactant are used: a. $4 \mathrm{Li}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Li}_{2} \mathrm{O}(s) \quad\left(\mathrm{Li}_{2} \mathrm{O}\right)$ b. $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{H}_{2} \mathrm{O}(l)$ (Fe) c. $\mathrm{Al}_{2} \mathrm{~S}_{3}(s)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{Al}(\mathrm{OH})_{3}(a q)+3 \mathrm{H}_{2} \mathrm{~S}(g) \quad\left(\mathrm{H}_{2} \mathrm{~S}\right)$

For each of the following reactions, calculate the grams of indicated product when $15.0 \mathrm{~g}$ of the first reactant and $10.0 \mathrm{~g}$ of the second reactant are used:
a. $4 \mathrm{Li}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Li}_{2} \mathrm{O}(s) \quad\left(\mathrm{Li}_{2} \mathrm{O}\right)$
b. $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{H}_{2} \mathrm{O}(l)$ (Fe)
c. $\mathrm{Al}_{2} \mathrm{~S}_{3}(s)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{Al}(\mathrm{OH})_{3}(a q)+3 \mathrm{H}_{2} \mathrm{~S}(g) \quad\left(\mathrm{H}_{2} \mathrm{~S}\right)$

Key Concepts

Stoichiometry

Stoichiometry is the branch of chemistry that involves calculating the amounts of reactants and products in chemical reactions using a balanced chemical equation. It requires understanding the mole relationships between substances and converting between mass and moles to predict product quantities or determine reactant requirements.

Molar Mass Conversion

Molar mass conversion involves using the molar mass of a substance to convert between the mass of a sample and the number of moles it contains. This calculation is essential for stoichiometric computations in chemical reactions, allowing chemists to relate the mass of reactants to the number of entities involved in the reaction.

Balanced Chemical Equations

Balanced chemical equations represent chemical reactions where the number of atoms for each element is the same on both the reactant and product sides. This balance is crucial for stoichiometric calculations, as it provides the mole ratio of reactants to products and helps identify the proportions in which substances react.

Limiting Reactant

The limiting reactant in a chemical reaction is the reactant that is entirely consumed first, limiting the amount of product that can be formed. Identifying the limiting reactant involves comparing the mole ratios of the available reactants to those required by the balanced equation, and it determines the theoretical yield of the reaction.

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