Question
Explain why the absolute values of the standard enthalpy change in the reaction and heat measured by the calorimeter are not equal. Assume that there are no measurement errors of any kind.
In the previous problem I solved that Delta H rxn was -1500 and q = 1.519 x 10^6 J and I said that it dealt with internal energy and got half credit. Can someone try to explain the theory to me?
In the previous problem I solved that Delta H rxn was -1500 and q = 1.519 x 10^6 J and I said that it dealt with internal energy and got half credit. Can someone try to explain the theory to me?