Chemistry enthalpy change of neutralisation

When doing calculations at A level to determine enthalpy change of neutralisation between an acid and an alkali you are given data of the volumes and concentrations of each reactant and the change in temperature during the reaction. I can work out the energy change (Q=mcT) however where I become stuck is working out the enthalpy change (Q/n). My problem is when the moles of the two reactants are different from each other, do you plug the smaller number of moles into the Q/n equation or do you plug the number of moles of water produced into the equation? Any help would be great and I hope that this made sense

do you plug the number of moles of water produced into the equation?

Do you have access to the answer? I would assume that the smallest number of moles and the moles of water produced would be the same if its a 1:1 neutralisation for example. Are you able to find a correlation between the smallest number of moles of reactant and the number of moles of water produced? I’m sorry im not too sure either now, I would assume use the mol of water

That.

If you have different mol of acid and base, see if one is in excess and use the limiting reagent to work out n(H2O) and plug that one in.