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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblema 45c
Capitolo 4, Problema 45c

For the reaction shown, calculate the theoretical yield of product (in grams) for each initial amount of reactants. 2 Al(s) + 3 Cl2(g) → 2 AlCl3(s) c. 0.235 g Al, 1.15 g Cl2

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Identify the balanced chemical equation: \(2 \text{Al}(s) + 3 \text{Cl}_2(g) \rightarrow 2 \text{AlCl}_3(s)\).
Calculate the molar mass of aluminum (Al) and chlorine gas (Cl2).
Convert the mass of each reactant to moles using their respective molar masses.
Determine the limiting reactant by comparing the mole ratio of the reactants to the coefficients in the balanced equation.
Calculate the theoretical yield of \(\text{AlCl}_3\) in grams using the moles of the limiting reactant and the molar mass of \(\text{AlCl}_3\).

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Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It involves using balanced chemical equations to determine how much of each substance is needed or produced. In this case, stoichiometry will help calculate the theoretical yield of aluminum chloride based on the given amounts of aluminum and chlorine.
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Percorso guidato
01:16
Stoichiometry Concept

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the theoretical yield, as it dictates how much product can be produced from the available reactants. In this scenario, one must determine whether aluminum or chlorine is the limiting reactant.
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Percorso guidato
01:30
Limiting Reagent Concept

Theoretical Yield

Theoretical yield is the maximum amount of product that can be generated from a given amount of reactants, assuming complete conversion and no losses. It is calculated using stoichiometric ratios derived from the balanced chemical equation. In this question, the theoretical yield of aluminum chloride will be calculated based on the limiting reactant and the initial masses of aluminum and chlorine.
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Percorso guidato
03:09
Percent Yield in Reactions
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Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

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Domanda del libro di testo

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

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Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) A reaction mixture initially contains 22.55 g Fe2O3 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

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For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F2( g) → TiF4(s) c. 0.233 g Ti, 0.288 g F2

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