# Problem: When a 4.25-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0 oC to 16.9 oC.You may want to reference (Pages 179 - 183) Section 5.5 while completing this problem.Assume that the specific heat of the solution is the same as that of pure water.Calculate delta(H) (in kJ/mol NH4NO3) for the solution proces.

###### FREE Expert Solution

Use the calorimetry equation to find the heat involved

Calculating the change in enthalpy for 1 mole ( MM of NH4NOis 80 g/mol)

96% (306 ratings) ###### Problem Details

When a 4.25-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0 oC to 16.9 oC. You may want to reference (Pages 179 - 183) Section 5.5 while completing this problem.

Assume that the specific heat of the solution is the same as that of pure water.

Calculate delta(H) (in kJ/mol NH4NO3) for the solution proces.

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Our tutors have indicated that to solve this problem you will need to apply the Constant-Pressure Calorimetry concept. You can view video lessons to learn Constant-Pressure Calorimetry. Or if you need more Constant-Pressure Calorimetry practice, you can also practice Constant-Pressure Calorimetry practice problems.