13.4 g of NH4Cl is dissolved in 150 mLof water in a coffee-cup calorimeter, and the temperature of the solution decreases from 24.80°C to 18.95°C. (a) Calculate the enthalpy change for the dissolution of this sample of NH4Cl in J. (b) What would be the enthalpy change for dissolving one mole of NH4Cl in kJ/mol? Note that the specific heat capacity of water is 4.186J/g·K and its density is 1.00 g/mL. Remember that the heat gained by the water is heat that is lost by the system.

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