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.

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10-06-2020
Chemistry

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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.

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mickymike92 mickymike92 · Answer 1 · 2020-06-10T07:36:15+02:00

Answer:

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.

bratislava bratislava · Answer 2 · 2022-01-21T14:30:19+01:00

bratislava bratislava

21-01-2022

As per the decomposition of the Ca(OH) 2 and the CaO the constant pressure needs to be added of the 109KJ.

The balance thermochemical equation for the reaction is expressed as Ca(OH)2 ----> Ca O + H2O; ∆H = +109KJ

The diagram for the reaction and the activation energy is given above.

Learn more about decomposition.

brainly.com/question/14797703.

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