Ch.6 Chemical Reactions: Mole and Mass Relationships

McMurry - Fundamentals of General, Organic, and Biological Chemistry 8th Edition

McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187당신이 사용하는 게 아니라요?교과서 변경

McMurry 8th Edition

Ch.6 Chemical Reactions: Mole and Mass Relationships

문제 53b

6장, 문제 53b

Nitrobenzene (C₆H₅NO₂) is used in small quantities as a flavoring agent or in perfumes but can be toxic in large amounts. It is produced by reaction of benzene (C₆H₆) with nitric acid:
C₆H₆(l) + HNO₃(aq) → C₆H₅NO₂(l) + H₂O(l)
b. Calculate the theoretical yield for this reaction.

검증된 단계별 안내

Step 1: Write the balanced chemical equation for the reaction. The given equation is already balanced:

C 6 H 6 (l) + H NO 3 (aq) \to C 6 H 5 NO 2 (l) + H 2 O (l)

Step 2: Determine the molar masses of the reactants and products. Use the periodic table to calculate the molar masses: Benzene (

C 6 H 6

) = 78.11 g/mol, Nitric acid (

H NO 3

) = 63.01 g/mol, Nitrobenzene (

C 6 H 5 NO 2

) = 123.11 g/mol.

Step 3: Identify the limiting reactant. To do this, calculate the number of moles of each reactant using the formula

n = \frac{m}{M}

, where

m

is the mass of the substance and

M

is its molar mass. Compare the mole ratio of the reactants to the stoichiometric ratio in the balanced equation.

Step 4: Calculate the theoretical yield of nitrobenzene. Use the mole ratio from the balanced equation to determine the moles of nitrobenzene that can be produced from the limiting reactant. Then, convert moles of nitrobenzene to grams using its molar mass:

m = n \times M

Step 5: Verify your calculations and ensure all units are consistent. Double-check the molar masses, mole ratios, and conversions to confirm the theoretical yield is accurate.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

도움이 되었나요?

주요 개념

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

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 the amounts of substances consumed and produced. In this case, understanding stoichiometry is essential for calculating the theoretical yield of nitrobenzene from benzene and nitric acid.

Theoretical Yield

Theoretical yield refers to the maximum amount of product that can be generated from a given amount of reactants, assuming complete conversion and no losses. It is calculated based on the stoichiometric coefficients from the balanced chemical equation. In this reaction, determining the theoretical yield of nitrobenzene requires knowing the initial amounts of benzene and nitric acid used.

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 of the product can be produced based on the initial quantities of reactants involved in the reaction.

Nitrobenzene (C6H5NO2) is used in small quantities as a flavoring agent or in perfumes but can be toxic in large amounts. It is produced by reaction of benzene (C6H6) with nitric acid:C6H6(l) + HNO3(aq) → C6H5NO2(l) + H2O(l)b. Calculate the theoretical yield for this reaction.

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Stoichiometry

Theoretical Yield

Limiting Reactant