dyke 270 Posted February 14, 2014 Share Posted February 14, 2014 So, this question was on my chemistry quiz and I'm positive that I got it wrong. Nitric acid is produced commercially by the Ostwald process represented by the following equation:4NH3(g) + 502(g)=> 4NO(g)+6H20(g)2NO(g)+ 02(g)=> 2NO2(g)3NO2(g)+ H20(g)=> 2HN03(aq) + NO(g)What masses of NH3 must be used to produce 1.0*10^6 kg HNO3 by the Ostwald process assuming 100% yield in each reaction. Sadly, this is a simplified version.... Link to comment Share on other sites More sharing options...
guava 6,874 Posted February 14, 2014 Share Posted February 14, 2014 I was going to type out an answer but I've used this in the past and it worked --->http://answers.yahoo.com/question/index?qid=20071019204323AAD8Q5N good luck Link to comment Share on other sites More sharing options...
ruppi 9,190 Posted February 14, 2014 Share Posted February 14, 2014 Why don't you just take the molar mass of 2HNO3 ? n= m/M ..that's all you need to do I think Oh wait I miss read ..brb Just read the above it's great Your ratio would be 2:1 Link to comment Share on other sites More sharing options...
takaminas 298 Posted February 14, 2014 Share Posted February 14, 2014 welp. i knew how to do this. >.< the process in that link should be easy to follow tho. good luck! i hated ap chem. welp. Link to comment Share on other sites More sharing options...
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