Chemical Equilibrium

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A reversible reaction is one where the products can react to reform the original reactants under the same conditions. It occurs simultaneously in both directions and reaches a dynamic equilibrium. Ex…

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Static equilibrium occurs when no movement or change takes place (e.g., book on a table). Dynamic equilibrium involves continuous forward and reverse processes at equal rates, so no net change is obse…

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In an open system, gaseous or volatile components may escape, preventing the reverse reaction from occurring. A closed system ensures all reactants and products remain, allowing equilibrium to be achi…

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At equilibrium, the forward and reverse reactions continue at equal rates, so concentrations remain constant. There is no net change, but reactions are ongoing. Example: In $$\mathrm{N_2O_4(g) \right…

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Yes, equilibrium can be reached whether starting with reactants or products. The same equilibrium constant applies. Example: Starting with pure $$\mathrm{N_2O_4}$$ or pure $$\mathrm{NO_2}$$, the same…

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The reaction is reversible and occurs in the presence of dilute H₂SO₄: $$\mathrm{CH_3COOH(l) + C_2H_5OH(l) \rightleftharpoons CH_3COOC_2H_5(l) + H_2O(l)}$$ This is a homogeneous liquid-phase equilib…

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The reaction is heterogeneous and occurs in a closed system: $$\mathrm{CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)}$$ Only CO₂ contributes to equilibrium constant expressions.

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The reaction is exothermic and involves gaseous species: $$\mathrm{N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)} \quad \Delta H = -92.4\ \mathrm{kJ/mol}$$ Used industrially under high pressure and l…