For a reaction with ΔH° = −9 kJ/mol, decide if the following statement is true. If it is false, choose the statement that makes it true. Select the single best answer. The reaction is exothermic. (Assume the reaction has a small entropy term compared to the enthalpy term) a. The statement is false. b. The reaction does not occur. c. The statement is true. d. The statement is false. e. The reaction is endergonic. f. The statement is false. g. The reaction is endothermic.

c. The statement is true

Explanation:

Endothermic reactions are defined as the reactions in which energy of the product is greater than the energy of the reactants. The total energy is absorbed in the form of heat and  for the reaction comes out to be positive.

Exothermic reactions are defined as the reactions in which energy of the product is lesser than the energy of the reactants. The total energy is released in the form of heat and  for the reaction comes out to be negative.

As the given value of , the heat is released and is exothermic.Thus the statement that the reaction is exothermic is true.

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