Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

6. Chemical Reactions & Quantities

Limiting Reagent

GOB Chemistry

6. Chemical Reactions & Quantities

Limiting Reagent

Previous problemNext problem

2:57 minutes

Problem 53b

Textbook Question

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.

Verified step by step guidance

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.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above

Video duration:

Play a video:

Was this helpful?

Key Concepts

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

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.

Watch next

Master Limiting Reagent with a bite sized video explanation from Jules

Start learning

Related Videos

Related Practice

Multiple Choice

The reaction between solid aluminum and iron (III) oxide can generate temperatures reaching 3000 ºC and is used in welding metals.

2 Al + Fe₂O₃ → Al₂O₃ + 2 Fe

If 150 g of Al are reacted with 432 g of Fe₂O₃, what is the mass of the excess reactant remaining?

Textbook Question

Consider the balanced chemical equation: 2A + B₂ → 2AB. Given the following reaction vessel, determine the theoretical yield of product.

<IMAGE>

1142

views

Textbook Question

In Problem 6.40, hydrazine reacted with oxygen according to the following (unbalanced) equation: N₂H₄(l) + O₂(g) → NO₂(g) + H₂O(g)

a. If 75.0 kg of hydrazine are reacted with 75.0 kg of oxygen, which is the limiting reagent?

1484

views

Textbook Question

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)

a. Identify the limiting reagent in the reaction of 27.5 g of nitric acid with 75 g of benzene.

1980

views

Textbook Question

Acetylsalicylic acid, the active ingredient in aspirin, is prepared from salicylic acid by reaction with acetic anhydride.

C₇H₆O₃ (salicylic acid) + C₄H₆O₃ (acetic anhydride) → C₉H₈O₄ (acetylsalicylic acid) + C₂H₄O₂ (acetic acid)

a. Calculate the theoretical yield if 47 g of salicylic acid is reacted with 25 g of acetic anhydride.

1820

views

Multiple Choice

Acrylonitrile (C₃H₃N) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction:

2 C₃H₆ (g) + 2 NH₃ (g) + 3 O₂ (g) → 2 C₃H₃N (g) + 6 H₂O (g)

If 12.0 g C₃H₆, 10.0 g NH₃, and 5.0 g O₂ react, what mass of acrylonitrile can be produced, assuming 100% yield?

The reaction between solid aluminum and iron (III) oxide can generate temperatures reaching 3000 ºC and is used in welding metals.

2 Al + Fe₂O₃ → Al₂O₃ + 2 Fe

If 150 g of Al are reacted with 432 g of Fe₂O₃, what is the mass of the excess reactant remaining?

Show more practices

Download the Mobile app

Privacy

Do not sell my personal information

Accessibility

Patent notice

Sitemap

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.

Key Concepts

Stoichiometry

Theoretical Yield

Limiting Reactant

Watch next