Search
- Filter Results
- Location
- Classification
- Include attachments
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/19%3A_Equilibrium/19.05%3A_Le_Chatelier's_PrincipleThis page explores two themes: the thrill of skydiving for stress relief through adrenaline, and Le Chatelier's Principle in chemistry, which explains how a chemical equilibrium reacts to external str...This page explores two themes: the thrill of skydiving for stress relief through adrenaline, and Le Chatelier's Principle in chemistry, which explains how a chemical equilibrium reacts to external stressors by shifting towards either the forward or reverse reaction, impacting the concentrations of reactants and products.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/19%3A_Equilibrium/19.02%3A_Chemical_EquilibriumThis page explains chemical equilibrium using the metaphor of a tug of war, where forces are equal but no movement occurs. It highlights the dynamic equilibrium in reactions like hydrogen iodide forma...This page explains chemical equilibrium using the metaphor of a tug of war, where forces are equal but no movement occurs. It highlights the dynamic equilibrium in reactions like hydrogen iodide formation, where forward and reverse reactions occur at equal rates, maintaining constant concentrations. Key conditions for equilibrium include a closed system and the presence of both reactants and products. It also mentions other forms of equilibrium, such as phase and solution equilibrium.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/19%3A_Equilibrium/19.01%3A_Reversible_ReactionThis page discusses the color change of cobalt chloride solutions due to solvated Co2+ ions, which turn pink, and shift to blue upon the addition of HCl forming \(\ce{CoCl_4^{2-}}...This page discusses the color change of cobalt chloride solutions due to solvated Co2+ ions, which turn pink, and shift to blue upon the addition of HCl forming CoCl2−4; this change can be reversed by adding water. It further explains reversible chemical reactions, exemplified by the formation and decomposition of hydrogen iodide from hydrogen and iodine, emphasizing that this process continues until a balance is reached between the forward and reverse reactions
