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 reaction, 2NH3 (g) → N2 (g) + 3H2( g) If the rate of hydrogen production is 0.030 mol L-1 s-1, then the rate of nitrogen production is a. 0.030 mol L-1 s-1b. 0.010 mol L-1 s-1c. 0.020 mol

Solution: Consider the reaction, 2NH3 (g) → N2 (g) + 3H2( g) If the rate of hydrogen production is 0.030 mol L-1 s-1, then the rate of nitrogen production is a. 0.030 mol L-1 s-1b. 0.010 mol L-1 s-1c. 0.020 mol

Problem

Consider the reaction, 2NH3 (g) → N2 (g) + 3H2( g) 

If the rate of hydrogen production is 0.030 mol L-1 s-1, then the rate of nitrogen production is 

a. 0.030 mol L-1 s-1

b. 0.010 mol L-1 s-1

c. 0.020 mol L-1 s-1

d. 0.090 mol L-1 s-1