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A 3.53–g sample of ammonium nitrate (NH4NO3) was added to
Chapter 6, Problem 78P(choose chapter or problem)
A 3.53-g sample of ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) was added to 80.0 mL of water in a constant pressure calorimeter of negligible heat capacity. As a result, the temperature of the water decreased from \(21.6^{\circ} \mathrm{C}\) to \(18.1^{\circ} \mathrm{C}\). Calculate the heat of solution \(\left(\Delta H_{\text {soln }}\right)\) of ammonium nitrate.
Questions & Answers
QUESTION:
A 3.53-g sample of ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) was added to 80.0 mL of water in a constant pressure calorimeter of negligible heat capacity. As a result, the temperature of the water decreased from \(21.6^{\circ} \mathrm{C}\) to \(18.1^{\circ} \mathrm{C}\). Calculate the heat of solution \(\left(\Delta H_{\text {soln }}\right)\) of ammonium nitrate.
ANSWER:Step 1 of 3
Here, we are going to calculate the heat of solution.
Given that,
Initial temperature,
Final temperature,
Mass of the sample = 3.53 g
Specific heat capacity, s = 4.184 J/gºC