Ch.13 - Chemical KineticsWorksheetSee 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

Identifying Reaction Order

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Sections
Rate of Reaction
Average Rate of Reaction
Arrhenius Equation
Rate Law
Integrated Rate Law
Collision Theory
Additional Practice
Instantaneous Rate of Change
Energy Diagram
Catalyst
Michaelis-Menten Equation
Reaction Mechanism
Identifying Reaction Order
Additional Practice

Solution: Consider the hypothetical reactionA + B + 2C → 2D + 3Ewhere the rate law isAn experiment is carried out where [A]0 = 1.0 x 10-2 M, [B]0 = 3.0 M, and [C]0 = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M.c. Calculate the concentration of A after 13.0 seconds.

Solution: Consider the hypothetical reactionA + B + 2C → 2D + 3Ewhere the rate law isAn experiment is carried out where [A]0 = 1.0 x 10-2 M, [B]0 = 3.0 M, and [C]0 = 2.0 M. The reaction is started, and after 8.

Problem

Consider the hypothetical reaction

A + B + 2C → 2D + 3E

where the rate law is

An experiment is carried out where [A]0 = 1.0 x 10-2 M, [B]0 = 3.0 M, and [C]0 = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M.

c. Calculate the concentration of A after 13.0 seconds.

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