Solid mercury(II) oxide decomposes into liquid mercury and oxygen gas upon the absorption of 90.8 kJ for each mole of mercury(II) oxide decomposed.​

The question is incomplete, the complete question is;

Solid mercury (II) oxide decomposes into liquid mercury and oxygen gas upon the absorption of 90.8 kJ for each mole of mercury (II) oxide decomposed.

What is the reaction without the energy?

What is the appropriate side of the equation and value for the energy term?

See Explanation

Explanation:

The equation of the reaction is;

2HgO(s) ==> 2Hg(l) + O2(g)

Let us recall that a chemical equation is balanced if the number of atoms of each element on both sides of the reaction equation are the same. There are two atoms each of mercury and oxygen on both sides of the reaction equation hence the equation is balanced.

In order to write a thermochemical equation, the heat of reaction is written on the right hand side of the reaction equation after writing the products as follows;

2HgO(s) ==> 2Hg(l) + O2(g)    ΔH = +90.8 kJ

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