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Which of the following statements is TRUE?a. The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants. b. The addition of a homogeneous catalyst does not change the activation energy of a given reaction. c. Rate constants are temperature dependent. d. None of the above is true. e. A catalyst raises the activation energy of a reaction.

Respuesta :

Answer:

The answer to the question which of the following statements is TRUE is

c. Rate constants are temperature dependent.

Explanation:

The rate constant can be derived from the following Arrhenius equation  thus

k = [tex]Ae^{-\frac{E_{a} }{RT} }[/tex]

Where A = Arrhenius constant

R = Universal gas constant

T= Absolute temperature

Eₐ = Activation energy of the reaction

The above equation makes it clear that the rate of a reaction is mainly impacted by the temperature of the reaction.

The rate constant therefore is not actually a constant as it is only valid for a specified temperature

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