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change of enthalpy by dissolving ammonium nitrate

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Please help answer the following thermodynamics questions.

a) When a 3.88g sample of solid ammonium nitrate dissolves in 60g of water in a coffee-cup calorimeter, the temperature drops from 23 degrees C to 18.4 degrees C.
Calculate ^H (in kJ/mol NH4NO3) for the solution process

NH4NO3(s)---->NH4(aq) + + NO3 -

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

b) Is this processes endothermic or exothermic?

Please show all work and define any symbols used--Thank you.

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Solution Summary

This posting helps with thermodynamic question. The solution shows how to calculate the change of enthalpy by dissolving ammonium nitrate. It also explains whether the process is endothermic or exothermic. Step by step calculations are given.

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a) When a 3.88g sample of solid ammonium nitrate dissolves in 60g of water in a coffee-cup calorimeter, the temperature drops from 23 degrees C to 18.4 degrees C.
Calculate ^H (in kJ/mol NH4NO3) for the solution process

First calculate the heat absobed by ...

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