Ch.3 - Chemical ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is C4H6O3 + C7H6O3 → C9H8O4 + C2H4O2In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g/ml) and 1.28 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the theoretical yield of aspirin for the reaction. Determine the percent yield of aspirin for the reaction.

Problem

Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is C4H6O3 + C7H6O3 → C9H8O4 + C2H4O2

In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g/ml) and 1.28 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. 

Determine the theoretical yield of aspirin for the reaction. 

Determine the percent yield of aspirin for the reaction.

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