What is the enthalpy of dissolution of NH4NO3?
What is the enthalpy of dissolution of NH4NO3?
25.7kJ/mol
As the ammonium nitrate dissolves, it absorbs heat from the body and helps to limit swelling. For ammonium nitrate, ΔHsoln=25.7kJ/mol. The molar heat of solution, ΔHsoln, of NaOH is −44.51kJ/mol.
What is the enthalpy change of ammonium nitrate?
| Enthalpy change of solution for some selected compounds | |
|---|---|
| hydrochloric acid | -74.84 |
| ammonium nitrate | +25.69 |
| ammonia | -30.50 |
| potassium hydroxide | -57.61 |
How do you calculate the enthalpy of a reaction?
Use the formula ∆H = m x s x ∆T to solve. Once you have m, the mass of your reactants, s, the specific heat of your product, and ∆T, the temperature change from your reaction, you are prepared to find the enthalpy of reaction. Simply plug your values into the formula ∆H = m x s x ∆T and multiply to solve.
What is the enthalpy of dissolution of CaCl2?
The enthalpy of dissolution of CaCl2 is −80 kJ/mol.
What is the chemical equation for the dissolving process of NH4NO3?
Question: The chemical equation for solid ammonium nitrate dissolving in 100 g of water is: NH4NO3(s) + NH4+ (aq) + NO3 (aq) To measure the enthalpy of this process, a calorimetry experiment was performed.
How to calculate enthalpy of dissolution in a calorimeter?
Assume that the calorimeter does not absorb any heat, that the density of the solution is the same as that of water ( 1 g m l − 1) and that the specific heat capacity of the solution is also the same as that of water ( 4.18 J g − 1 K − 1).
What is the standard enthalpy of dissolution of ammonium nitrate?
Even before doing any calculations, you can look at the change in temperature measured for the water to say that you can expect the standard molar enthalpy of dissolution of ammonium nitrate to be positive.
How many moles in a sample of ammonium nitrate?
If you look at things from water’s perspective, you can say that water gives off heat, hence the negative sign. Now, the standard molar enthalpy of dissolution is usually expressed in kilojoules per mole. Use ammonium nitrate’s molar mass to determine how many moles you get in that sample
How to calculate enthalpy change in kJ mol?
In a polystyrene cup calorimeter, 4.3 g of ammonium nitrate, NHX4NO, was added to 60.0 g of water and stirred to dissolve the solid completely. The initial temperature dropped from 22.0 ∘ C to a final temperature of 16.9 ∘ C. Calculate the enthalpy change in kJ mol − 1 for this dissolution process,…