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How do you determine the enthalpy change of neutralization between HCl and NaOh?
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∙ 13y ago
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∙ 13y ago
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What is the aim of a thermometric titration?
the aim of a thermometric titration is to determine the concentration of the titrand and also to calculate the enthalpy change of neutralization.
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.
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.
Why is the enthalpy change of neutralisation equal to -57.2kJ mol-1?
Actually your question should sound "Why is the enthalpy change of neutralization of STRONG ACID and STRONG BASE equal to -57.2kJmol-1?". This is because when STRONG ACID and STRONG BASE react and neutralization process occur, a complete ionization will occur. Therefore, they will have almost the same value of enthalpies and can be assummed to be -57.2kJmol-1. As per mentioned that if your question sounds "Why is the enthalpy change of neutralization of STRONG ACID and STRONG BASE equal to -57.2kJmol-1?", then my explaination above will be helpful. However, if it doesn't sound like mine and you insisted with your question titled "Why is the enthalpy change of neutralization equal to -57.2kJmol-1", then my answer is that they didn't equal to -57.2kJmol-1 and it varies from the list of reactants. 1. STRONG acid + STRONG base = -57.2 2. WEAK acid + WEAK base = less than 57.3kJmol-1 3. WEAK acid + STRONG base = more negative than -57.3kJmol-1 Wish that it is useful as your reference. Prompt me if I am wrong.
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 aim of a thermometric titration?
the aim of a thermometric titration is to determine the concentration of the titrand and also to calculate the enthalpy change of neutralization.
Why is the standard enthalpy change of neutralization between hydrofluoric acid and sodium hydroxide more negative than usual?
Because of high of heat of Hydration of HF ( Fluoride ion is extensively hydrated because of it's small size )
What is relation between hydration energy lattice energy and enthalpy of solution?
enthalpy change of solution=enthalpy change of hydration - enthalpy change of lattice
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.
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.
Why is the enthalpy change of neutralisation equal to -57.2kJ mol-1?
Actually your question should sound "Why is the enthalpy change of neutralization of STRONG ACID and STRONG BASE equal to -57.2kJmol-1?". This is because when STRONG ACID and STRONG BASE react and neutralization process occur, a complete ionization will occur. Therefore, they will have almost the same value of enthalpies and can be assummed to be -57.2kJmol-1. As per mentioned that if your question sounds "Why is the enthalpy change of neutralization of STRONG ACID and STRONG BASE equal to -57.2kJmol-1?", then my explaination above will be helpful. However, if it doesn't sound like mine and you insisted with your question titled "Why is the enthalpy change of neutralization equal to -57.2kJmol-1", then my answer is that they didn't equal to -57.2kJmol-1 and it varies from the list of reactants. 1. STRONG acid + STRONG base = -57.2 2. WEAK acid + WEAK base = less than 57.3kJmol-1 3. WEAK acid + STRONG base = more negative than -57.3kJmol-1 Wish that it is useful as your reference. Prompt me if I am wrong.
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
How does the presence of a catalyst affect the enthalpy change of a reaction?
The presence of a catalyst affect the enthalpy change of a reaction is that catalysts do not alter the enthalpy change of a reaction. Catalysts only change the activation energy which starts the reaction.
What does the different in potential energy between the reactant and products represent?
It represents the change in enthalpy for the reaction.
What is molar enthalpy change?
Molar bond enthalpy shows the change in a bond association. For example, if one mole of bond is broken, the energy change that results is DHd (degree).
How can the enthalpy change be determined for a reaction in an aqueous solution?
Utilizing a thermometer to measure the temperature change of the solution can be used (along with the mass of the reactant(s)) to determine the enthalpy change for an aqueous reaction, as long as the reaction is carried out in a calorimeter or similar apparatus so that no external heat is added or removed from the system.
What is to change from solid to a gas and vice versa?
Enthalpy of Vaporization and Enthalpy of Condensation.
