0
What is the enthalpy of neutralization (delta Hn) per mole of H2SO4/Ba(OH)2 is?
Mushfiqua memon
Want this question answered?
Be notified when an answer is posted
Add your answer:
Earn +20 pts
What do the symbols mean Delta Hr Hf Hc Hn Ha in chemistry btw i know theyre enthalpy changes?
delta Hr is the enthalphy change of a reaction delta Hf is the enthalpy of formation where one mole of a substance is formed ( generally in its naturally occurring physical state) delta Hc is the enthalpy of combustion where one mole of a substance in its standard state undergoes combustion delta Hn is the enthalpy of neutralization where one mole of H+ reacts with OH- to form one mole of H2O delta Ha is the enthalpy of atomization where a molecule splits to form its neutral atomic components
What is the heat of neutralization of nitric acid?
The Enthalpy of neutralization of all strong acids are almost the same. It is between -58 to -59 kilojoules per mole.
Definition for standard enthalpy change of neutralization?
Enthalpy change of neutralisation is defined as the enthalpy change of a reaction where one mole of hydrogen ions reacts with one mole of hydroxide ions to form one mole of water under standard conditions of 1 atm, 298K (25 degree Celsius) and in the solutions containing 1 mol per dm3.
What is the difference between enthalpy change and enthalpy change per mole?
Enthalpy is the energy absorbed or lost from a reaction, but enthalpy change per mole is the amount of energy lost per mole, so in order to get the overall enthalpy from the change per mole, you must multiply that value by the amount of moles used in the reaction.
What is standard enthalpy change of atomization?
the breaking down of elements into atoms. it is the energy required when 1 mole of a substance completely decomposes into its gaseous atoms i.e endothermic reaction, delta H is +ve meaning breaking bonds
What is the enthalpy change of neutralisation for strong acid with a strong base?
The enthalpy of neutralization of a strong acid against a strong base is always constant (13.7 kcal or 57 kJ mole-1). It is because in dilute solutions all strong acids and bases ionize completely and thus the heat of neutralization in such cases is actually the heat of formation of water from H+ and OH- ions, i.e., H+ + OH- ---> H2O; ΔH = -13.7 kcal
What is the equation of heat of hydration?
Heat of hydration or enthalpy of hydration of ions corresponds to the heat that is released by hydration of one mole of ions at a constant pressure. The more the ion is hydrated, the more heat is released. Degree of hydration depends on the size and charge of ion. The smaller the ion and the greater its charge, it will be the more hydrated.
Will exactly one mole of calcium hydroxide neutralize exactly one mole of phosphoric acid?
No, because one mole of calcium hydroxide constitutes two equivalents of calcium hydroxide for neutralization, but one mole of phosphoric acid constitutes three equivalents of phosphoric acid for neutralization. Therefore, one mole of calcium hydroxide will neutralize only 2/3 of one mole of phosphoric acid.
What is the standard molar enthalpy of formation for ammonium chloride aq?
-299.65 kJ/mole
How do I convert the enthalpy of vaporization of water in joules per gram from kiloJoules per mole?
Lets say, for example the enthalpy is equal to 1200 joules/gram. You take 1200 joules/gram * (# of grams)/one mole [now you can cancel grams and it is now joules/mole.] Then convert the answer to kilojoules by dividing by 1000.
What is the enthalpy change for dissolution of one mole of ammonium nitrate?
+25.69 kJ mol-1
How does lattice energy differs from bond enthalpy?
Bond enthalpy is the energy required to break a chemical bond whereas lattice energy is the enthalpy of formation of one mole of an ionic compound from gaseus ions under standard conditions.
