The enthalpy change of the neutralisation given below is –114 kJ mol–1.2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l) By using this information, what is the most likely value for the enthalpy change of the following neutralisation?
Definition of the enthalpy change of neutralization: the energy released with the formation of 1 mole of water when neutralization takes place between an acid and a base. Since both reactions yield the same number of moles of water, the answer should be C. Hope this makes sense
Definition of the enthalpy change of neutralization: the energy released with the formation of 1 mole of water when neutralization takes place between an acid and a base. Since both reactions yield the same number of moles of water, the answer should be C. Hope this makes sense
My explanation was 'same number of moles for reactants and products.' Thank you anyways!