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

Solution: Consider the reaction3A + B + C → D + Ewhere the rate law is defined asAn experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 1.00 x 10-4 M.c. Calculate the concentration of B and the concentration of A after 10.0 min.

Solution: Consider the reaction3A + B + C → D + Ewhere the rate law is defined asAn experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 1.00 x 10-4 M.c. Calculate the concentration of B and the conc

Problem

Consider the reaction

3A + B + C → D + E

where the rate law is defined as

An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 1.00 x 10-4 M.

c. Calculate the concentration of B and the concentration of A after 10.0 min.