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: In a study of the decomposition of nitramide in aqueous solution at 25°C.NH2NO2 (aq) → N2O (g) + H2O (l) the concentration of NH2NO2 was followed as a function of time. It was found that a graph of ln

Problem

In a study of the decomposition of nitramide in aqueous solution at 25°C.

NH2NO(aq) → N2O (g) + H2O (l) 

the concentration of NH2NO2 was followed as a function of time. It was found that a graph of ln[NH2NO2] versus time in seconds gave a straight line with a slope of -6.72 x 10-5 s-1 and a y-intercept of -0.863. 

Based on this plot, the reaction is ________ order in NH2NO2 and the rate constant for the reaction is _____________ s-1.