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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 38
Chapter 4, Problem 38

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O2( g) → 2 Al2O3(s)
a. 1 mol Al, 1 mol O2
b. 4 mol Al, 2.6 mol O2
c. 16 mol Al, 13 mol O2
d. 7.4 mol Al, 6.5 mol O2

Verified step by step guidance
1
Identify the balanced chemical equation: 4 Al(s) + 3 O_2(g) → 2 Al_2O_3(s).
For each scenario, calculate the mole ratio of Al to O_2 based on the balanced equation, which is 4:3.
a. Calculate the amount of Al needed to react with 1 mol of O_2 using the ratio: (4 mol Al / 3 mol O_2) * 1 mol O_2.
b. Calculate the amount of O_2 needed to react with 4 mol of Al using the ratio: (3 mol O_2 / 4 mol Al) * 4 mol Al.
Compare the calculated amounts with the given amounts to determine the limiting reactant for each scenario.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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. To identify it, one must compare the mole ratio of the reactants used in the reaction to the coefficients in the balanced chemical equation.
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Limiting Reagent Concept

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It involves using mole ratios derived from the coefficients of the balanced equation to determine how much of each reactant is needed or how much product can be formed from given amounts of reactants.
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Mole Ratio

Mole ratio is the ratio of moles of one substance to the moles of another substance in a balanced chemical equation. It is essential for converting between moles of reactants and products, allowing chemists to predict how much of each reactant is required or how much product will be produced in a reaction.
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Related Practice
Textbook Question

Calculate the theoretical yield of the product (in moles) for each initial amount of reactants.

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b. 7 mol Ti, 17 mol Cl2

c. 12.4 mol Ti, 18.8 mol Cl2

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Consider the reaction: 4 HCl(g) + O2(g) → 2 H2O(g) + 2 Cl2(g) Each molecular diagram represents an initial mixture of reactants. How many molecules of Cl2 form from the reaction mixture that produces the greatest amount of products?

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For each of the acid–base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 4.85 g of the base. b. 2 HNO3(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(NO3)2(aq)

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Textbook Question

Find the limiting reactant for each initial amount of reactants.

2 Na(s) + Br2(g) → 2 NaBr(s)

a. 2 mol Na, 2 mol Br2

b. 1.8 mol Na, 1.4 Br2

c. 2.5 mol Na, 1 mol Br2

d. 12.6 mol Na, 6.9 mol Br2

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Textbook Question

Consider the reaction: 2 CH3OH(g) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) Each of the molecular diagrams represents an initial mixture of the reactants. How many CO2 molecules form from the reaction mixture that produces the greatest amount of products?

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