A 1 mol sample of `N_(2)(g)` reacts with 1 mol of `O_(2)(g)` to form 2 mol of NO(g),, where the increase in enthalpy is 180.6 kJ. Draw an enthalpy diagramm for this reaction.

Explanation

`N_(2)(g)+O_(2)(g) to 2NO(g),DeltaH=+180.6kJ`
In the reaction, the enthalpy increases. So, it is an endothermic reaction. In such a reaction the total enthalpy of the product(s) `(sumH_(P))` is greater than that of the reactant(s) `(sumH_(R))`. therefore, in the enthalpy diagram for the reaction, `sumH_(P)` lies above `sumH_(R)`.
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