If the activation energy required for a chemical reaction were reduced, what would happen to the rate of the reaction
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The relation between rate of reaction and activation energy is given by Arrhenius equation : k = Ae^-Ea/RT
We can see that as activation energy decrease, rate increases in an exponential manner.
Conceptually, we can think of the activation energy as a hill in front of the reactants. For the reactants to become products, energy is required to go over the hill. Higher the hill, higher the energy, lesser products. Hence, by decreasing activation energy, we are reducing the height of the hill and making it easier for reactants to become products.
We can see that as activation energy decrease, rate increases in an exponential manner.
Conceptually, we can think of the activation energy as a hill in front of the reactants. For the reactants to become products, energy is required to go over the hill. Higher the hill, higher the energy, lesser products. Hence, by decreasing activation energy, we are reducing the height of the hill and making it easier for reactants to become products.
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The rate of reaction will increase in an exponential order.
In chemistry and physics, activation energy is the amount of energy which must be provided to a chemical or nuclear system with potential reactants to result in: a chemical reaction, nuclear reaction, or various other physical phenomena.
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