1. The problem statement, all variables and given/known data Decomposition of 2 moles of NH4NO3 at 100 degrees C.calculate work done 2. Relevant equations NH4NO3 (s)→N2O(g)+2H2O (g) work done= - RT delta n here R=universal gas constant T=temperature in kelvin and delta n=difference in number of moles of products and reactants. 3. The attempt at a solution-I pluged in the values in formula work done= - RT delta n =- 8.314j per kelvin per mol×373 kelvin ×3 mol =- 9303.366 j I took delta n =3 because i think delta number of moles in solid phase is taken as zero.Even if i don't number of moles in solid phase =0 rather I Take number of moles in solid phase = 1, I will get delta n =2 and then work done= - RT delta n =- 8.314 j per kelvin per mol ×373 kelvin ×2 mol =- 6202.244 j But according to my textbook answer should be - 18.61kj please help.