High Quality Content by WIKIPEDIA articles! The standard enthalpy change of neutralisation is the change in enthalpy that occurs when an acid and base undergo a neutralisation reaction to form one mole of water under standard conditions (298 K and 1 atm), i.e. react to produce water and a salt. It is a special case of the standard enthalpy change of reaction. Equations for working out standard enthalpy of neutralisation: Q = mc?T Where: * Q is the heat energy liberated * m is the mass of the solution. * c is the specific heat capacity of the solution. * ?T is the temperature change of the reaction between an acid and a base. From this the standard enthalpy change (?H) can be calculated by dividing the negative of Q by the moles of the limiting reactant, usually moles of H+ ions. The standard enthalpy change of neutralisation for a strong acid and base is -57.3 kJ/mol. ?h=-q/n in kJmol-1 The standard enthalpy of mineral acids is far greater than that of organic acids. This is because strong acids ionise completely and yet organic acids ionise partially.

Данное издание не является оригинальным. Книга печатается по технологии принт-он-деманд после получения заказа.