The decomposition of Ca(OH)2(s) intoCaO(s) and H2O(g) at constant pressure requires the addition of 109 kJ of heat per mole of Ca(OH)2. A. Write a balanced thermochemical equation for the reaction.
B. Draw an enthalpy diagram for the reaction, showing the activation energy, Ea, and the enthalpy change for the reaction.

A. Ca(OH)2 > CaO + H2O; ∆H = +109KJ

B. Check attached document below for the enthalpy diagram

Explanation:

A thermochemical equation is a balanced chemical equation in which enthalpy change is variable. It tells about the nature of the reaction.

Enthalpy change is the difference between the heat content of the products and reactants in a thermochemical equation.

∆H is negative for an exothermic reaction (a reaction where heat is given out), while it is positive for an endothermic reaction ( a reaction in which heat is added).

The activation energy, Ea, is the minimum amount of energy reactant particles must possess in order for a reaction to proceed towards product formation.

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explanation:

because u need two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei to form isotopes.

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