The true statement about this chemical reaction is that: D. the change in enthalpy is +180 kJ, so it is an endothermic reaction.
In order to determine whether this chemical reaction is endothermic or exothermic, we would determine the change in enthalpy as follows:
The change in enthalpy = The energy of products - the energy of reactants
Substituting the given parameters into the formula, we have;
The change in enthalpy = -240 - (-420)
The change in enthalpy = -240 + 420
The change in enthalpy = 180 kJ.
Since the change in enthalpy for this chemical reaction, we can infer and logically conclude that it is an endothermic reaction because heat is absorbed.
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Complete Question:
The table shows the thermodynamic data for a reaction.
Thermodynamic Data:
Energy of the Reactants: -420 kJ
Energy of the Products: -240 kJ
Activation Energy: -310 kJ
Which of the following statements explains if the reaction is endothermic or exothermic?
The activation energy is lower than the change in enthalpy, so it is an exothermic reaction.
B. The activation energy is higher than the change in enthalpy, so it is an endothermic reaction.
C. The change in enthalpy is -180 kJ, so it is an exothermic reaction.
D. The change in enthalpy is +180 kJ, so it is an endothermic reaction.
