CHEM 101A Chapter Notes - Chapter 6-7: Equilibrium Constant, Ideal Gas Law, Exothermic Reaction
3 Nov 2016
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Document Summary
Some reactions are fast because they have low energy of activation. Some reactions are slow because they have high energy of activation. Reactions that form products that are lower in energy than the reactants can have high activation energy. Increasing concentration of reactants increases number of collisions so reaction rate increases. Increasing temp increases kinetic energy which increases number of collisions. Increasing temp increases average kinetic energy of reactants because kinetic energy of colliding molecules is used for bond cleavage, more molecules have enough energy. Some reactions don"t occur in a reasonable period of time without a catalyst. A substance that speeds up a reaction rate. Accelerates a reaction by lowering the energy of activation is recovered unchanged in a reaction that it does not appear in the product. No effect on energies of reactants and products. Adding a catalyst lowers activation energy or delta h. Metals are often used as catalyst reactions.
