dorcus Posted October 16, 2005 Share Posted October 16, 2005 I was just wondering if Barium Hydroxide + Ammonium Chloride would be a dangerous endothermic reaction. Link to comment Share on other sites More sharing options...
RyanJ Posted October 16, 2005 Share Posted October 16, 2005 I was just wondering if Barium Hydroxide + Ammonium Chloride would be a dangerous endothermic reaction. Well, I'll probably not be able to help much bere because i'm not shure what is formed when they react If, however, you know what the products of the reaction are then you can work out the total bond energy to start with and take the end bond energy from that, if you get a negative value then its exothermic, otherwise its endothermic Good luck, Ryan Jones Link to comment Share on other sites More sharing options...
woelen Posted October 16, 2005 Share Posted October 16, 2005 I was just wondering if Barium Hydroxide + Ammonium Chloride would be a dangerous endothermic reaction. When mixed, these give NH3, H2O and BaCl2. I would expect this to be an exothermic reaction, although not a really strong exothermic reaction. Endothermic reactions are not dangerous at all (at least not in terms of violence, heat, ignition, explosion etc.). Link to comment Share on other sites More sharing options...
akcapr Posted October 16, 2005 Share Posted October 16, 2005 This reacton is endothermic, itsn not dangerous unless you drink it. Its alot like BaOH and AN, it can freeze water. Link to comment Share on other sites More sharing options...
RyanJ Posted October 16, 2005 Share Posted October 16, 2005 Endothermic reactions are not dangerous at all (at least not in terms of violence' date=' heat, ignition, explosion etc.).[/quote'] Isn't the decomposition of [ce]NI_3[/ce] endothermic? I'm shure I read somewhere it was? Cheers, Ryan Jones Link to comment Share on other sites More sharing options...
woelen Posted October 16, 2005 Share Posted October 16, 2005 Can you give me a reference? I hardly can imagine that this reaction is endothermic, but of course you may be right. I never studied the NI3/NH3 system in detail. The only reason, where an endothermic reaction may be dangerous is where solid compounds are converted to gaseous compounds at high speed, but I do not know an example of an endothermic reaction with that property. Link to comment Share on other sites More sharing options...
RyanJ Posted October 16, 2005 Share Posted October 16, 2005 Can you give me a reference? I hardly can imagine that this reaction is endothermic' date=' but of course you may be right. I never studied the NI3/NH3 system in detail. The only reason, where an endothermic reaction may be dangerous is where solid compounds are converted to gaseous compounds at high speed, but I do not know an example of an endothermic reaction with that property.[/quote'] I'm pretty shure it was here Cheers, Ryan Jones Link to comment Share on other sites More sharing options...
budullewraagh Posted October 16, 2005 Share Posted October 16, 2005 i think dorcus was talking about the efflorescence of the octahydrate of barium hydroxide taking effect and dissolving the ammonium chloride, which is indeed an endothermic process Link to comment Share on other sites More sharing options...
jdurg Posted October 17, 2005 Share Posted October 17, 2005 The decomposition of NI3 is DEFINITELY not endothermic. The Nitrogen-Iodine bond is not very strong, but the Nitrogen-Nitrogen triple bond is VERY strong. Energy is released when bonds are formed, so the formation of that N-N triple bond releases far more energy than the breaking of the N-I bonds require. Also, you completely misred the quote here: The process 2 NI3 (s) => N2 (g) + 3 I2 (s) is exothermic, so that N2 (g) + 3 I2 (s) => 2 NI3 (s) is endothermic. Endothermic compounds tend to be unstable. What that is stating is that HEAT OF FORMATION of NI3 is endothermic. The enthalpy of reaction for the decomposition of NI3 is quite exothermic. Link to comment Share on other sites More sharing options...
RyanJ Posted October 17, 2005 Share Posted October 17, 2005 Also' date=' you completely misred the quote here: [/quote'] Yea, it looks like - thanks for the correction Cheers, Ryan Jones Link to comment Share on other sites More sharing options...
dorcus Posted October 17, 2005 Author Share Posted October 17, 2005 thanks guys budellwraagh, that's exactly what i was talking about Link to comment Share on other sites More sharing options...
woelen Posted October 17, 2005 Share Posted October 17, 2005 I'm pretty shure it was here Cheers' date=' Ryan Jones[/quote'] The process 2 NI3 (s) N2 (g) + 3 I2 (s) is exothermic, so that N2 (g) + 3 I2 (s) 2 NI3 (s) is endothermic. Endothermic compounds tend to be unstable. I have the idea that you misinterpreted this sentence. The compound is endothermic, so the decomposition is exothermic. EDIT woelen: Sorry, jdurg already pointed out this reading-error. Link to comment Share on other sites More sharing options...
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