Skip to main content
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 37b
4장, 문제 37b

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?

검증된 단계별 안내
1
Identify the balanced chemical equation: 4 \(\text{HCl}\)(g) + \(\text{O}\)_2(g) \(\rightarrow\) 2 \(\text{H}\)_2\(\text{O}\)(g) + 2 \(\text{Cl}\)_2(g)
Determine the stoichiometric ratios from the balanced equation: 4 moles of HCl react with 1 mole of O_2 to produce 2 moles of Cl_2.
Examine the initial mixture of reactants to identify the limiting reactant by comparing the available moles of HCl and O_2.
Calculate the maximum number of Cl_2 molecules that can be formed based on the limiting reactant using the stoichiometric ratio.
Verify the calculation by ensuring that the number of Cl_2 molecules formed does not exceed the amount predicted by the stoichiometry of the reaction.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
5m

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It allows us to determine the proportions of each substance involved in the reaction, which is essential for predicting how much product will form from given amounts of reactants.
추천 영상:
가이드 코스
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 yield of products, as it dictates how far the reaction can proceed.
추천 영상:
가이드 코스
01:30
Limiting Reagent Concept

Molecular Ratios

Molecular ratios are derived from the coefficients of a balanced chemical equation and indicate the relative amounts of reactants and products involved in the reaction. Understanding these ratios is vital for predicting the quantities of products formed from specific amounts of reactants, particularly in determining how many molecules of Cl<sub>2</sub> can be produced.
추천 영상:
가이드 코스
02:14
Neutron-Proton Ratio
관련 실천
교과서 질문

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

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

1693
views
교과서 질문

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

3 Mn(s) + 2 O2(g) → Mn3O4(s)

a. 3 mol Mn, 2 mol O2

b. 4 mol Mn, 7 mol O2

c. 27.5 mol Mn, 43.8 mol O2

3761
views
1
rank
교과서 질문

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

3015
views
1
comments
교과서 질문

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

2817
views
1
rank
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)

3460
views
교과서 질문

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?

2725
views
1
comments