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The larger this ratio, the smaller the rate (hence the negative sign.) This means that high temperature and low activation energy favor larger rate constants, and thus speed up the reaction. And because these terms occur in an exponent, their effects on the rate are quite substantial. Therefore, temperature has to be considerably large to have an effect with a low activation energy. If activation energy is low, a greater proportion of the collisions between reactants will result in reactions. If the temperature of the system is increased, the average heat energy is increased, a greater proportion of collisions between reactants result in reaction, and the reaction proceeds more rapidly. A catalyst increases the reaction rate by providing a reaction mechanism with a lower activation energy, so that a greater proportion of collisions result in reaction.
Yes. Essentially, because the activation energy is low already, not that much extra kinetic energy is needed to start the reaction, so increasing temperature (and therefore kinetic energy) does not do that much for the reaction
If the amount of energy that is needed to make a reaction happen is small, then no matter how much you raise temperature, the reaction will occur regardless because it only needs a small increase in order to occur.
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