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$Chemical equilibrium is an important concept in chemistry that explains how reversible reactions behave when the rate of the forward reaction becomes equal to the rate of the reverse reaction. 1. Chemical Reaction A chemical reaction is a process in which reactants change into products. Example: 2H_2 + O_2 \rightarrow 2H_2O Hydrogen reacts with oxygen to form water. 2. Types of Chemical Reactions A. Irreversible Reaction A reaction that proceeds only in one direction. Characteristics Products do not convert back into reactants. Reaction goes to completion. Represented by a single arrow (→). Example NaOH + HCl \rightarrow NaCl + H_2O B. Reversible Reaction A reaction that proceeds in both forward and reverse directions. Characteristics Products can change back into reactants. Represented by double arrows (⇌). Establishes equilibrium. Example N_2 + 3H_2 \rightleftharpoons 2NH_3 3. Forward and Reverse Reactions Forward Reaction Reaction in which reactants form products. N_2 + 3H_2 \rightarrow 2NH_3 Reverse Reaction Reaction in which products convert back into reactants. 2NH_3 \rightarrow N_2 + 3H_2 At equilibrium: \text{Rate of Forward Reaction} = \text{Rate of Reverse Reaction} 4. Chemical Equilibrium Chemical equilibrium is the state at which the rate of the forward reaction becomes equal to the rate of the reverse reaction. \text{Rate of Forward Reaction} = \text{Rate of Reverse Reaction} Important Points Occurs only in reversible reactions. Concentrations become constant. Reaction does not stop. Equilibrium can be disturbed by changing conditions. --- 5. Dynamic Nature of Equilibrium Equilibrium is dynamic because: Forward reaction continues. Reverse reaction also continues. Both reactions occur at equal rates. Example In a closed bottle of water: Water evaporates. Vapor condenses back. Eventually equilibrium is established. --- 6. Law of Active Masses The law of active masses states: > “The rate of a chemical reaction is directly proportional to the product of active masses (concentrations) of reactants.” Example aA + bB \rightleftharpoons cC + dD According to the law: Forward rate: R_f \propto [A]^a[B]^b Reverse rate: R_r \propto [C]^c[D]^d At equilibrium: [A]^a[B]^b = [C]^c[D]^d --- 7. Equilibrium Constant (Kc) The equilibrium constant is the ratio of product concentrations to reactant concentrations at equilibrium. For reaction: aA + bB \rightleftharpoons cC + dD K_c=\frac{[C]^c[D]^d}{[A]^a[B]^b} Important Points Products are written in numerator. Reactants are written in denominator. Powers are equal to coefficients. Pure solids and liquids are not included. --- 8. Units of Kc Units depend on the reaction. Example 1 H_2 + I_2 \rightleftharpoons 2HI K_c = \frac{[HI]^2}{[H_2][I_2]} Units cancel out. Unit: No unit --- Example 2 N_2 + 3H_2 \rightleftharpoons 2NH_3 K_c = \frac{[NH_3]^2}{[N_2][H_2]^3} Unit: dm^6mol^{-2} --- 9. Values of Kc If Kc > 1 Products are favored. More products formed. If Kc < 1 Reactants are favored. Few products formed. If Kc = 1 Equal amounts of reactants and products. --- 10. Recognition of Equilibrium Physical Methods A. Refractometer Measures refractive index changes. B. Polarimeter Measures rotation of plane polarized light. C. Spectrophotometer Measures light absorption by substances. --- Chemical Method Titration Used to measure concentration changes during reaction. When concentration becomes constant, equilibrium is reached. 21. Short Summary Chemical equilibrium is a dynamic state of reversible reactions where forward and reverse reaction rates become equal. The equilibrium position depends on concentration, pressure, volume, and temperature according to Le Chatelier’s Principle. Equilibrium constant (Kc) helps determine the extent of reaction and direction of equilibrium. 👉 Follow for more easy content! or join our Whatsapp channel👇👇👇👇 https://whatsapp.com/channel/0029Vb7uiP0AYlUNkzs66y0o #Aspire_Coaching_Academy #Malakand #chemistry #chemicalequilibrium #1MillionViewsOnMyFirstVideo$
Chemical equilibrium is an important concept in chemistry that explains how reversible reactions behave when the rate of the forward reaction becomes equal to the rate of the reverse reaction. 1. Chemical Reaction A chemical reaction is a process in which reactants change into products. Example: 2H_2 + O_2 \rightarrow 2H_2O Hydrogen reacts with oxygen to form water. 2. Types of Chemical Reactions A. Irreversible Reaction A reaction that proceeds only in one direction. Characteristics Products do not convert back into reactants. Reaction goes to completion. Represented by a single arrow (→). Example NaOH + HCl \rightarrow NaCl + H_2O B. Reversible Reaction A reaction that proceeds in both forward and reverse directions. Characteristics Products can change back into reactants. Represented by double arrows (⇌). Establishes equilibrium. Example N_2 + 3H_2 \rightleftharpoons 2NH_3 3. Forward and Reverse Reactions Forward Reaction Reaction in which reactants form products. N_2 + 3H_2 \rightarrow 2NH_3 Reverse Reaction Reaction in which products convert back into reactants. 2NH_3 \rightarrow N_2 + 3H_2 At equilibrium: \text{Rate of Forward Reaction} = \text{Rate of Reverse Reaction} 4. Chemical Equilibrium Chemical equilibrium is the state at which the rate of the forward reaction becomes equal to the rate of the reverse reaction. \text{Rate of Forward Reaction} = \text{Rate of Reverse Reaction} Important Points Occurs only in reversible reactions. Concentrations become constant. Reaction does not stop. Equilibrium can be disturbed by changing conditions. --- 5. Dynamic Nature of Equilibrium Equilibrium is dynamic because: Forward reaction continues. Reverse reaction also continues. Both reactions occur at equal rates. Example In a closed bottle of water: Water evaporates. Vapor condenses back. Eventually equilibrium is established. --- 6. Law of Active Masses The law of active masses states: > “The rate of a chemical reaction is directly proportional to the product of active masses (concentrations) of reactants.” Example aA + bB \rightleftharpoons cC + dD According to the law: Forward rate: R_f \propto [A]^a[B]^b Reverse rate: R_r \propto [C]^c[D]^d At equilibrium: [A]^a[B]^b = [C]^c[D]^d --- 7. Equilibrium Constant (Kc) The equilibrium constant is the ratio of product concentrations to reactant concentrations at equilibrium. For reaction: aA + bB \rightleftharpoons cC + dD K_c=\frac{[C]^c[D]^d}{[A]^a[B]^b} Important Points Products are written in numerator. Reactants are written in denominator. Powers are equal to coefficients. Pure solids and liquids are not included. --- 8. Units of Kc Units depend on the reaction. Example 1 H_2 + I_2 \rightleftharpoons 2HI K_c = \frac{[HI]^2}{[H_2][I_2]} Units cancel out. Unit: No unit --- Example 2 N_2 + 3H_2 \rightleftharpoons 2NH_3 K_c = \frac{[NH_3]^2}{[N_2][H_2]^3} Unit: dm^6mol^{-2} --- 9. Values of Kc If Kc > 1 Products are favored. More products formed. If Kc < 1 Reactants are favored. Few products formed. If Kc = 1 Equal amounts of reactants and products. --- 10. Recognition of Equilibrium Physical Methods A. Refractometer Measures refractive index changes. B. Polarimeter Measures rotation of plane polarized light. C. Spectrophotometer Measures light absorption by substances. --- Chemical Method Titration Used to measure concentration changes during reaction. When concentration becomes constant, equilibrium is reached. 21. Short Summary Chemical equilibrium is a dynamic state of reversible reactions where forward and reverse reaction rates become equal. The equilibrium position depends on concentration, pressure, volume, and temperature according to Le Chatelier’s Principle. Equilibrium constant (Kc) helps determine the extent of reaction and direction of equilibrium. 👉 Follow for more easy content! or join our Whatsapp channel👇👇👇👇 https://whatsapp.com/channel/0029Vb7uiP0AYlUNkzs66y0o #Aspire_Coaching_Academy #Malakand #chemistry #chemicalequilibrium #1MillionViewsOnMyFirstVideo

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