Enthalpy of Solution?

Question

Please help by providing an equation and reasoning.

In a coffee-cup calorimeter, 1.40 g of NH4NO3 was mixed with 74.0 g of water at an initial temperature of 25.00°C. After dissolution of the salt, the final temperature of the calorimeter contents was 23.71°C.

(a) Assuming the solution has a heat capacity of 4.18 J/g°C, and assuming no heat loss to the calorimeter, calculate the enthalpy of solution (Delta Hsoln) for the dissolution of NH4NO3 in units of kJ/mol.

b)(b) If the enthalpy of hydration for NH4NO3 is -630. kJ/mol, calculate the lattice energy of NH4NO3.

Thanks.

Answer 1

Molar mass of NH4NO3 = 14+4+14+48 = 80

So, 1.4 g is equal to 1.4/80 = 0.0175 mol

Now, mass of soln = 74+1.4 g = 75.4 g

So, heat absorbed = 75.4x4.18x(25-23.71) = 404.415 J

So, 0.0175 mol absorbs 404.415 J

So, 1 mol absorbs 23109.429 J

So, heat of dissolution of NH4NO3 is 23.109 kJ/mol (+ve as heat is absorbed)

b) Lattice energy = 630+23.109 = 653.109 kJ/mol

Answer 2

Enthalpy Of Solution

Answer 3

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RE:
Enthalpy of Solution?
Please help by providing an equation and reasoning.

In a coffee-cup calorimeter, 1.40 g of NH4NO3 was mixed with 74.0 g of water at an initial temperature of 25.00°C. After dissolution of the salt, the final temperature of the calorimeter contents was 23.71°C.

(a) Assuming the solution...

Answer 4

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Not quite, the enthalpy of solution is one of the three dimensions of solubility analysis. So it is one variable, but not enough to determine solubility