A common chemistry demonstration is to dissolve ammonium nitrate into water. In a particular demonstration, 8.53 grams of ammonium nitrate were dissolved in 100.00 mL of water. As a result, the temperature of the solution dropped from 25.0 oC to 19.0 oC. Calculate q of the solution in Joules (assume m to be the total mass of solution).

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Beverley SmithLv2

17 Feb 2019

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Part 1:

A common chemistry demonstration is to dissolve ammonium nitrate into water. In a particular demonstration, 5.61 grams of ammonium nitrate were dissolved in 100.00 mL of water. As a result, the temperature of the solution dropped from 25.0 oC to 20.9 oC. Calculate q of the solution in Joules (assume m to be the total mass of solution).

Part 2:

How many moles of ammonium nitrate were dissolved in the solution?

Part 3:

Which of the following represents the sign of ÎHsoln of ammonium nitrate. In other words, which represents the sign of ÎH for the below process:

NH4NO3(s) âNH4(aq) + NO3(aq)

Negative, because the process releases heat

Positive, because the process releases heat

Positive, because the process absorbs heat

Negative, because the process absorbs heat

Part 4:

Calculate the ÎHsoln of ammonium nitrate. In other words, calculate ÎH (in kJ/mol) for the below process:

NH4NO3(s) âNH4(aq) + NO3(aq)

4. Instant cold packs are used for first aid when ice is not available. In one such device, a small pouch containing 2x102 grams of ammonium nitrate (NH4NO3) is placed in a bag containing 2x102 milliliters of water initially at 25oC. When the pouch is broken, ammonium nitrate dissolves in the water and the cold pack reaches a final temperature of -2oC. i). Calculate âHos (kJ/mol NH4NO3) for the solution in the cold pack, assuming that the pack loses negligible amount of heat to the surroundings during the dissolution process and that the heat capacity of the solution is that of pure water. ii). What would be the final temperature (oC) of a pack containing 300 grams of ammonium nitrate and 300 ml of water? Show work

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