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Original post by X_301
NH4Cl (s) ------> NH3 (g) +HCl (g)
Suggest why the enthalpy change for reaction is difficult to determine directly by experiment ?
Suggest why the enthalpy change for reaction is difficult to determine directly by experiment ?
Well this is a decomposition. You would heat it and a significant proportion of that heat would be lost to the surroundings, no matter how well you insulated it. It may also require specialist equipment to get it to high enough temperatures. The compound is likely to have impurities in it. You would never get every single gram of it to decompose.
There are too many variables to try and control, that's why Hess's law and Born-Haber cycles are rather nice methods!
(edited 6 years ago)
Original post by _NMcC_
Well this is a decomposition. You would heat it and a significant proportion of that heat would be lost to the surroundings, no matter how well you insulated it. It may also require specialist equipment to get it to high enough temperatures. The compound is likely to have impurities in it. You would never get every single gram of it to decompose.
There are too many variables to try and control, that's why Hess's law and Born-Haber cycles are rather nice methods!
There are too many variables to try and control, that's why Hess's law and Born-Haber cycles are rather nice methods!
Thank you
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