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# When 2 moles of potassium chlorate crystals decompose to potassium chloride crystals and oxygen gas at constant temperature and pressure, 44.7 kJ are given off. What is the thermochemical equation?

##2"KClO"_text(3(s]) -> 2"KCl"_text((s]) + 3"O"_text(2(g]). " "DeltaH_text(rxn) = -"44.7 kJ"##

A **thermochemical equation** is simply a chemical equation that contains information about the change of reaction, ##DeltaH_"rxn"##.

The first thing to do when writing a thermochemical equation is to make sure that you get the balnced chemical equation right.

In your case, you know that **2 moles** of potassium chlorate, ##"KClO"_3##, undergo to form potassium chloride, ##"KCl"##, and oxygen gas, ##"O"_2##.

So you know that you have

##2"KClO"_text(3(s]) -> "KCl"_text((s]) + "O"_text(2(g])##

Balance this equation by multiplying the products by ##2## and ##3##, respectively

##2"KClO"_text(3(s]) -> 2"KCl"_text((s]) + 3"O"_text(2(g])##

Now focus on the enthalpy change of reaction. The problem tells you that the reaction **given off** ##"44.7 kJ"##, which means that the reaction is actually .

As you know, energy changes are being represent from the point of view of the system. This implies that for an exothermic reaction the enthalpy change will carry a **negative sign**, since the system is losing heat to the surroundings.

Therefore, the enthalpy change of reaction will be

##DeltaH = -"44. 7 kJ"##

As a result, the thermochemical equation for the decomposition of potassium chlorate looks like this

##2"KClO"_text(3(s]) -> 2"KCl"_text((s]) + 3"O"_text(2(g]). " "DeltaH_text(rxn) = -"44.7 kJ"##