Answer :
The rate constant for the reaction at 17.0°C is 0.010 s^-1, and its activation energy is 35.8 kJ/mol.
What is the significance of the rate constant and activation energy in the reaction?
The rate constant is a crucial parameter in determining the rate of a chemical reaction. It represents the proportionality constant between the concentrations of reactants and the rate of the reaction. In this case, the rate constant is 0.010 s^-1, indicating that for every second, a fraction of the reactants will be converted into products.
The activation energy, on the other hand, represents the minimum energy required for the reactant molecules to undergo the necessary collision and form products. In this case, the activation energy is 35.8 kJ/mol, indicating that the reaction requires a significant amount of energy to proceed.
The rate constant and activation energy are related through the Arrhenius equation, which states that the rate constant is exponentially dependent on the activation energy and temperature. A higher activation energy leads to a slower reaction rate, while a lower activation energy leads to a faster reaction rate.
Learn more about activation energy
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