Ch.13 - Chemical KineticsWorksheetSee all chapters
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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: At a certain temperature, the half-life of the first order decomposition of phenol (shown below) is 1.94 hr. phenol → cyclopentadiene + carbon monoxide Answer the following questions about the decomposition of phenol and report all answers to three significant figures. 1. If the initial concentration of phenol is 4.89 times 10-4 M, calculate the time (in hr) required for the concentration of phenol to decrease to 27.5% of the initial concentration. 0.896 hr 2. If the initial concentration of phenol is 4.89 times 10-4 M, calculate the concentration (in M) after 1.48 hr. 2.82*10-5 M

Problem

At a certain temperature, the half-life of the first order decomposition of phenol (shown below) is 1.94 hr.

phenol → cyclopentadiene + carbon monoxide

Answer the following questions about the decomposition of phenol and report all answers to three significant figures.

1. If the initial concentration of phenol is 4.89 times 10-4 M, calculate the time (in hr) required for the concentration of phenol to decrease to 27.5% of the initial concentration. 0.896 hr

2. If the initial concentration of phenol is 4.89 times 10-4 M, calculate the concentration (in M) after 1.48 hr. 2.82*10-5 M


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