The Δ Hrxn, in kJ/mol, for this reaction= 11.04 kJ/mol
Further explanation
Given
0.848 g ammonium nitrate
The enthalpy change : +0.117 kJ
Required
Δ Hrxn, in kJ/mol
Solution
Delta H reaction (ΔH) is the amount of heat change between the system and its environment
The value of ° H ° can be calculated from the change in enthalpy of standard formation:
∆H ° rxn = ∑n ∆Hf ° (product) - ∑n ∆Hf ° (reactants)
mass of NH4NO3 = 0.848 g
mol of NH4NO3(MW = 80 g/mol)
mol = 0.848 : 80
mol = 0.0106
The Δ Hrxn :
= 0.117 kJ : 0.0106 mol
= 11.04 kJ/mol
