Answer:
The rate constant increases for an increase in tempature and as activation energy increases the rate constant decreases.
Explanation:
Now since the rate constant increases this implies that the rate of reaction increases in tempature.
When activation energy of the reaction increases, rate constant of the reaction decreases.
Activation energy is the minimum amount of energy which is required to convert the reacting molecules into product.
Rate constant is the value which is equal to the ratio of the rate of the reaction to the concentration of reactants as:
k = Rate / Concentration of reactants
Activation energy is inversely proportional to the rate of the reaction and relation will be shown by the following equation:
[tex]k = Ae^{-Ea/RT}[/tex]
From the above two reactions it is clear that on increasing activation energy, rate constant of the reaction decreases.
Hence, the rate constant decreases as activation energy increases.
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