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: Enter your answer in the provided box. Hydrogen sulfide decomposes according to the following reaction, for which Kc = 9.30 x 10-8 at 700°C: 2H2S (g) ⇌ 2H2 (g) + S2 (g)If 0.49 mol of H2S is placed in

Problem

Enter your answer in the provided box. 

Hydrogen sulfide decomposes according to the following reaction, for which 

Kc = 9.30 x 10-8 at 700°C: 

2H2S (g) ⇌ 2H2 (g) + S2 (g)

If 0.49 mol of H2S is placed in a 3.0-L container, what is the equilibrium concentration of H2(g) at 700°C?