Measurement of Enthalpy example problem in course reader

[juliana alden 2D]

In the course reader, the example given reads "In a constant P calorimeter at 25ºC mix 50.0ml each of 1.0M HCl and 1.0 NaOH Afte Mixing T=39ºC
How much heat is released-Assume density of Soln is 1.0 g/ml (PURE WATER) and use specific heat capacity of water, 4.18 J/(ºC*g)"

What if the Molarity of the reactants HCl and NaOH weren't 1.0M? Is it still possible to solve the problem with the given information and, if so, how? Thanks!

[Kanwaldeep Rai 2H]

I believe you can still do the problem but you would have to account for the fact that the concentration of one reactant is more than another and thus only a certain amount of H2O can be produced. I think this would become a limiting reactant problem because the mole ratio of reactant to product is one. H+ + OH- -> H2O. So if there was 1 mol of HCl and 2 moles of NaOH, you could still only produce 1 mol of H2O.