To determine the enthalpy change for the forward reaction and whether it is endothermic or exothermic, we need to understand the relationship between bond breaking and bond forming.
In a chemical reaction:
- Energy is required to break bonds in the reactants, which is endothermic (absorbs energy).
- Energy is released when new bonds are formed in the products, which is exothermic (releases energy).
Given the options, we see that the enthalpy change for the forward reaction is -2,328 kJ/mol. A negative enthalpy change indicates that the reaction releases energy, which means it is exothermic.
The correct answer would describe the reaction as releasing energy because energy is produced from the formation of new bonds in the products.
Among the options provided:
C. -2,328 kJ/mol, exothermic because energy is released when forming bonds in the products.
This option correctly states that the reaction is exothermic and explains the reason accurately.
3 answers