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: CoCl42-(aq, blue) + 6H2O(l) ⇌ Co(H2O)62-(aq, pink) + 4Cl-(aq) [REVERSIBLE EQ.]QUESTION: When the pink equilibrium solution formed from CoCl2 was placed in a hot water bath, the solution turned blue. W

Problem

CoCl42-(aq, blue) + 6H2O(l) ⇌ Co(H2O)62-(aq, pink) + 4Cl-(aq) [REVERSIBLE EQ.]

QUESTION: When the pink equilibrium solution formed from CoCl2 was placed in a hot water bath, the solution turned blue. When placed into an ice bath, it turned back to pink. Cite specific observation results to identify the forward reaction in this equilibrium as an exothermic, or as an endothermic process. Write an equation for this equilibrium depicting heat as a reactant or producr of the reaction.

Solution
  • According to Le Chatelier’s Principle if a system (chemical reaction) is at equilibrium and we disturb it then the system will readjust to maintain its equilibrium state
  • For this reaction, the pink solution containing Co(H2O)62- is produced upon dissolving of CoCl2
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