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: The reaction of 11.9 g of CHCl3 with excess chlorine produced 11.2 g of CCl4, carbon tetrachloride:What is the percent yield?A. 94%B. 36.4%C. 100%D. 48.5%E. 72.8%

Problem

The reaction of 11.9 g of CHCl3 with excess chlorine produced 11.2 g of CCl4, carbon tetrachloride:

What is the percent yield?

A. 94%

B. 36.4%

C. 100%

D. 48.5%

E. 72.8%

Solution

Establish the balanced equation of the reaction of CHCl3 and CCl4 and use stoichiometry to determine the actual yield and eventually the percent yield

The balanced equation of CHClwith Cl2 will appear as:

CHCl+ Cl→ CCl4 + HCl

Recall that percent yield is given by:

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