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

Q = mCTQ = (60 g)(4.18 Jg°C)(22°C-16.9°C)Q = 1279 J

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

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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.

A diagram shows two Styrofoam cups nested together.  The inside cup contains the reaction mixture in solution, and is covered by a cork stopper, through which a thermometer and glass stirrer are placed.

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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