When 12.5 g of NH4NO3 is dissolved in 150.0 g of water of 25.0 °C in a coffee cup calorimeter, the final temperature of the solution of 19.7 °C. Assume that the specific heat of the solution is the same as that of water, 4.18 J/(g•°C). What is the ΔH per mol of NH4NO3? (LO 9.10)
NH4NO3 (s) → NH4+ (aq) + NO3−(aq) ΔH = ?
(a) +3.60 kJ
(b) +23.0 kJ
(c) +21.3 kJ
(d) −3.60 kJ
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?
Master Heat Capacity with a bite sized video explanation from Jules Bruno