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Ch.4 - Chemical Reactions and Chemical Quantities
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 5th EditionCh.4 - Chemical Reactions and Chemical Quantities문제 36
4장, 문제 36

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

검증된 단계별 안내
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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주요 개념

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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.
추천 영상:
가이드 코스
01:30
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.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept

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.
추천 영상:
가이드 코스
02:14
Neutron-Proton Ratio
관련 실천
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Ti(s) + 2 Cl2(g) → TiCl4(s)

a. 4 mol Ti, 4 mol Cl2

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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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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교과서 질문

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

a. 2 K(s) + Cl2(g) → 2 KCl(s)

b. 2 K(s) + Br2(l) → 2 KBr(s)

c. 4 Cr(s) + 3 O2(g) → 2 Cr2O3(s)

d. 2 Sr(s) + O2(g) → 2 SrO(s)

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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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