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Reaction Coordinate Activation Energy
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Activation Energy: • Definition: Activation energy (Ea) is the minimum amount of energy required for a chemical reaction to occur. It represents the energy barrier that reactant molecules must overcome to transform into products. • Units: Activation energy is typically expressed in joules (J) or kilojoules per mole (kJ/mol). • Role: Activation energy is a crucial factor in determining the rate of a chemical reaction. Reactions with higher activation energies proceed more slowly because a larger energy input is needed to initiate the reaction. • Temperature Dependence: The rate of reaction increases exponentially with temperature due to the Arrhenius equation, which relates rate constant (k), activation energy (Ea), and temperature (T): k = Ae^(-Ea/RT), where R is the gas constant. • Reaction Profiles: Activation energy is depicted on potential energy diagrams (reaction profiles) as the energy difference between the reactants and the transition state (activated complex), which is the highest energy point on the diagram. • Catalysis: Catalysts lower the activation energy of a reaction by providing an alternative reaction pathway, making reactions proceed faster. • #science101 #activationenergy #catalyst #chemicalreaction #organicchemistry #reactioncoordinate #reactionrate #chemistry #scienceshorts #homeschoolcurriculum #sciencefacts
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