Use the ΔHrxn values of the following reactions: 2SO2(g) + O2(g) → 2SO3(g) ΔHrxn = –196 kJ 2S(s) + 3O2(g) → 2SO3(g) ΔHrxn = –790 kJ to calculate the ΔHrxn value of this reaction: S(s) + O2(g) → SO2(g) ΔHrxn = ?

The for the reaction is -297 kJ.

Explanation:

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

The intermediate balanced chemical reaction are:

(1)    

(2)     

The expression for enthalpy of the reaction follows:

Putting values in above equation, we get:

Hence, the for the reaction is -297 kJ.

if you mean hydrogen and oxygen then water is the product

a compound is a molecule made of atoms from different elements.

a. by the combination of an unlimited number of elements