-299.65 kJ/mole
The enthalpy of formation of aqueous potassium chloride is approximately -436.1 kJ/mol. This value represents the energy change when 1 mole of potassium chloride is formed in its standard state from its elements in their standard states at 25°C and 1 atm.
I dont exactly know what the difference between the books are but you follow the standard procedure, using Q=mc(delta)T, where c is the specific heat of hcl and naoh, you can say that you assume the hcl and naoh take on the properties of water unless you know hwo to calculate it. Hope that helps
[from wikipedia] The standard enthalpy of formation"standard heat of formation" of a compound is the change of enthalpy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 degrees Celsius). Its symbol is ΔHfO.
The calculated value might be -281.86 kcal/mol or 1179.3 J/mol. See Ref: J. Chem. Educ., 1965, 42 (9), 474
The standard heat/enthalpy of formation of SO2 is -296.8 KJ
The enthalpy of formation for NH4Cl (ammonium chloride) is -314.4 kJ/mol. This means that when one mole of NH4Cl is formed from its elements in their standard states, 314.4 kJ of heat is released.
The enthalpy of formation of aqueous potassium chloride is approximately -436.1 kJ/mol. This value represents the energy change when 1 mole of potassium chloride is formed in its standard state from its elements in their standard states at 25°C and 1 atm.
The standard enthalpy of formation for N2 gas is 0 kJ/mol.
The standard enthalpy of formation is the energy change when one mole of a compound is formed from its elements in their standard states. The standard enthalpy of reaction is the energy change for a reaction under standard conditions. The relationship between the two is that the standard enthalpy of reaction is the sum of the standard enthalpies of formation of the products minus the sum of the standard enthalpies of formation of the reactants.
Oxygen gas (O2) does not have an enthalpy of formation because it is an element in its standard state, which has an enthalpy of formation of zero by definition. Ozone (O3), on the other hand, is a compound and has a defined enthalpy of formation because it is formed from its elements in their standard states.
The standard enthalpy for sodium sulphate is -1387kJ/mol.
The standard enthalpy of formation for sodium chloride is -411,12 kJ/mol.
The reaction is exothermic; the standard enthalpy of formation for sodium chloride is -411,12 kJ/mol at 25 0C.
The standard enthalpy of formation of coconut oil is not a well-defined value as it is a complex mixture of triglycerides, which are composed of various fatty acids. The enthalpy of formation of each individual fatty acid can be determined, but not for coconut oil as a whole.
Enthalpy of combusion is energy change when reacting with oxygen. Enthalpy of formation is energy change when forming a compound. But some enthalpies can be equal.ex-Combusion of H2 and formation of H2O is equal
The standard enthalpy of formation for potassium hydroxide is -425,8 kJ/mol.
You shouldn't "calculate" a standard enthalpy of formation. The beauty of standard enthalpies of formation is that they are already calculated for you. That is why they are delineated by the term "standard" - they are standards that were figured out by chemists some time ago, that never change, and can be found in tables usually in textbooks and even on Wikipedia. If you need to know the standard enthalpy of formation of FeO, Google it. And let me know what you find...because I can't seem to find a set answer either. I have found one site that lists the standard enthalpy of formation of FeO to be 271.9 kJ/mol. But it hasn't been so evident in other places. No wonder you were confused! Good luck.