Ch.14 - Chemical EquilibriumWorksheetSee 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: Nitrogen gas can spontaneously combine with hydrogen gas to create hydrazine based on the following reaction:                                                  N     2 (g)  +  2 H2 (g) ⇌ N2H4 (g)                                     What is the Kc for the forward reaction if the equilibrium concentrations of N 2, H2 and N2H4 are 0.800 atm, 0.500 atm and 0.010 atm respectively at 25oC ? 

Solution: Nitrogen gas can spontaneously combine with hydrogen gas to create hydrazine based on the following reaction:                                                  N     2 (g)  +  2 H2 (g) ⇌ N2H4 (g)    

Problem

Nitrogen gas can spontaneously combine with hydrogen gas to create hydrazine based on the following reaction:

                                                 N     2 (g)  +  2 H2 (g) ⇌ N2H4 (g)                                    

What is the Kc for the forward reaction if the equilibrium concentrations of N 2, H2 and N2H4 are 0.800 atm, 0.500 atm and 0.010 atm respectively at 25oC ?