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 following reaction: H2(g) + Br2(g) → 2HBr. The graph below shows the concentration of Br2 as a function of time.Use the graph to calculate the instantaneous rate of formation of HBr at 50

Problem

Consider the following reaction: H2(g) + Br2(g) → 2HBr. The graph below shows the concentration of Br2 as a function of time.
A graph of time, in seconds, versus concentration, in molars. The initial concentration is one molar, then decraeses linearly at a rate of point one molar per ten seconds for the first thirty seconds. It then begins to curve with upward concavity, having a concentration of point six molar at fifty seconds.

Use the graph to calculate the instantaneous rate of formation of HBr at 50 s.