Commercial cold packs consist of solid nh4no3 and water. in a coffee-cup calorimeter, 5.60g nh4no3 is dissolved in 100g of water at 22.0c; the temperature falls to 17.9c. assuming that the specific heat capacity of the solution is 4.18 j/(g*k), calculate the enthalpy of dissolution of nh4no3, in kj/mol.

-1.37 kJ/mol

Explanation:

The expression for the calculation of the enthalpy of dissolution of [tex[NH_4NO_3[/tex] is shown below as:-

Where,  

 is the enthalpy of dissolution of [tex[NH_4NO_3[/tex]

m is the mass

C is the specific heat capacity

 is the temperature change

Thus, given that:-

Mass of ammonium nitrate = 5.60 g

Specific heat = 4.18 J/g°C

So,  

Negative sign signifies loss of heat.  

Also, 1 J = 0.001 kJ

So,  

Also,

Molar mass of [tex[NH_4NO_3[/tex] = 80.043 g/mol

The formula for the calculation of moles is shown below:

Thus,

Thus,

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