Ammonium nitrate (MW = 80) is used in ‘cold packs’ to give a cooling effect for sports injuries. The solid crystals are added to water producing an endothermic reaction. A typical ‘cold pack’ contains 40 g of ammonium nitrate that is dissolved in water to make 200 g of the solution. Calculate the molar concentration of the ammonium nitrate solution and hence the drop in temperature that occurs when this pack is used.

[1 mole of ammonium nitrate dissolved in water to make 1 kg of solution produces a drop in temperature of 6.2 °C]

### 1 Answer | Add Yours

Ammonium nitrate dissolves in water in an endothermic reaction.

A typical ‘cold pack’ contains 40 g of ammonium nitrate that is dissolved in water to make 200 g of the solution.

We know 80 g NH4NO3 when dissolved in water to make 1000 ml solution is 1.0 M.

Therefore, 40 g NH4NO3 dissolved in water to make 200 ml solution would be 1.0*1000*40/(80*200) = **2.5 M**. This is the molarity of salt in the cold pack.

Further, 1 mole of ammonium nitrate when dissolved in water absorbs sufficient heat that produces a temperature drop of 6.2 degrees Celsius of the 1 kg solution that is produced.

The typical ‘cold pack’ contains half the amount of salt in one-fifth volume of solution. Therefore, this amount of NH4NO3 upon dissolution would absorb sufficient heat to produce a temperature drop of 6.2*5/2 = **15.5 degrees Celsius**.

**Sources:**

### Join to answer this question

Join a community of thousands of dedicated teachers and students.

Join eNotes