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Which of the following statements is incorrect concerning the thermochemical equation below? 2SO3(g) → 2SO2(g) + O2(g); ΔH° = 198 kJ a. The enthalpy of the reactants exceeds that of the products. b. For the reaction 2SO2(g) + O2(g) → 2SO3(g), ΔH° = –198 kJ. c. The reaction is endothermic. d. The external pressure is 1 atm. e. For every mole of SO3(g) consumed, 99 kJ of heat at constant pressure is consumed as well.

Respuesta :

Answer:

The incorrect statement is a.

Explanation:

[tex]2SO_3(g)\rightarrow 2SO_2(g)+O_2(g)[/tex] ΔH° = 198 kJ

Endothermic reactions are defined as the reactions in which energy is absorbed by the chemical reaction.The enthalpy of the reaction [tex](\Delta H)[/tex] positive.

This can be also understood as the reactions in which the energy of products is more than the energy of the reactants.

In the given thermochemical equation,enthalpy of the products exceeds that of the reactants

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