1. The problem statement, all variables and given/known data Given the reaction K2CO3(s) + 2HCl(aq) → 2KCl(aq) + CO2(g) + H2O(l), I need to find the enthalpy change in J, given that: The specific heat capacity of water is 4.2J g-1 °C-1, and The mass change of potassium carbonate is 2.98g, and the temperature change was °6C, and the volume of acid used was 30cm3. 2. Relevant equations ΔH = -qmΔT number of moles of acid neutralised = number of moles of water formed 3. The attempt at a solution Considering it is a neutralisation reaction, I did the ΔH = -qmΔT equation. So, -4.2x-2xm=x x/(2x0.03) But what do I use for m?