# Calorimetry | Heat produced VS Change of enthalpy

There are two questions on the same test paper.

1. Calculate the amount of heat energy, $q$, produced in the reaction
2. Find the change of heat ($-q$).

I'm not sure whether or not they mean the same thing, but I highly doubt it seeing as though they would have the same answer, but as I said, I'm not sure. In question 1 I know that the reaction is exothermic and therefore is a negative value, for question 2 I do the same thing and get the same value. Do these questions have different meanings or are they both a quick way to getting easy marks?

## 1 Answer

I think that in the first question, as they ask you to calculate the amount of heat produced during the reactions, you need to write a positive value. The change of heat has a negative value for exothermic reactions. For example: In a reaction, the change of heat is -100 kJ/mol, then you can conclude that the reaction is exothermic. Therefore the heat produced in this reaction is 100 kJ/mol. When you say "the heat produced is" you don't write a minus sign.