So I have been facing a few difficulties in understanding the effect of the concentration of an acid excess has on the enthalpy change of a displacement and neutralisation reactions.
So imagine that we have 2 beakers of HCl both containg the same amount of the limiting reactant, let's say Magnesium ium for instance, and I am concerned of calculating the enthalpy change of the reaction, so in the beaker where the acid was more concentrated the temperature increase will be higher which results in greater amount of energy released, thus increasing the enthalpy change as the same number of moles of magnesium is reacting.
How come the enthalpy change is the same for the reaction ?
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Enthalpy change. watch
- Thread Starter
- 21-09-2017 06:15
- Official Rep
- 27-09-2017 04:16
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