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.

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 =

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

here is table 2-2:

country

percent of eligible voters that voted

rank

united states

44.9%

138

canada

60.1%

107

costa rica

84.6%

14

hungary

66.9%

82

japan

57.0%

118

egypt

27.7%

159

south africa

85.5%

10

ans is no, the data set cannot be plotted as a single circle graph