I need molybdate nitrite. Can i know your capacity on this chemical.?
153959
are you a frickin a pyro
924787
First of all\n3 moles of NO2 give you 2 moles of HNO3, while 1 mol of water gives you the same amount of product. We must find out which reactant gives you the least product, and that will be your maximum amount of product.\n36,0g H2O*(1mol H2O/18g H2O)*(2moles HNO3/1mol H2O)*(63g HNO3/1mol HNO3)= 252 g of HNO3\n\nNow with NO2\n92,0g NO2*(1mol NO2/46g NO2)*(2 moles HNO3/ 3moles NO2)*(63g HNO3/1mol HNO3)= 84,0g HNO3\nTherefore, the biggest amount of HNO3 you can expect to get is 84,0g.
871578
http://www.olysun.com/Chem_121/Soln.html\n\n\ncc
679263
I think that what is troubling you could be an exerecise involving "molarity" which uses two quantities: mass(moles)/volume(liter). \nBut you have to bear in mind that mass is referred to the solute, and volume refers to the solution. So, these quantities are not referring to ONE substance. \nIt would be better if you posted a question with the whole exercise, for clarity. \nGood luck.
1101057
2N2H4 + N2O4 -> 3N2 + 4H2O\n\nn(N2H4) = 3.125 mol\nn(N2O4) = 3.333 mol\n\nAs 2mol N2H4 rx c 1mol N2O4, n(N2H4rxn) = 1.563mol, and hence it is the limiting reactant. n(N2O4) = n(N2) = 1:3\nTherefore, 1.563 * 3 = 4.688 mol of Nitrogen gas, which equates to 131.25g.
622147
Wow dude you'll probably blow yourself up if you succeed.\nYou would probably be able to make it by continuing the nitration of TNT with a very powerful nitrating agent - say, nitronium tetrafluroborate.  But I don't think you will make it.
412358
You could skip the Nitrogen Oxide and use Nitrous Oxide.   :o)
291470
Yes, you are correct. The atomic number of Molybdenum is 42.
955612
In2(MoO4)3\noxidation number of Mo is +6
799105
Assume you have the salt AxBy and the molar solubility is s.\n\nThen\n\nAxBy <=> xA^(+y) +yB(^-x)\ns mole/lt\ngive... .. .. ..xs .. .. .. ..ys\n\nKsp=([A(+y)]^x) *[B(-x)]^y =(xs)^x * (ys)^y=>\nKsp= (x^x)*(y^y)*s^(x+y)\n\ne.g. for Fe3(PO4)2 tou have x=3, y=2, so\nKsp=(3^3)*(2^2)*s^(3+2)= 36s^5
876235
The product of a neutrilization reaction is always water and a salt, so use that as a guide.  For part 2, use the units as a guide.  Hint M=molarity=mols/L
373250
C3H7NO2 \n\nwww.chemfinder.com is a useful resource.  \n\nI hope this helps :)
550619
Most strong oxidizers are going to be potentially explosive.  What are you trying to oxidize?\n\nOctanitrocubane has some serious kick though.
42193
http://www.itt.edu/staff/boyter/links/index.html\n\nLook under chemistry equipment.  There are some chemicals you will not be able to get.  Posting what you are looking for would help.
881865
Since you didn't say what results you desire it is not really possible for anyone to answer your question.\n\nBut KNO3, potassium nitrate, commonly called "salt peter", is an oxidizing agent used in gun powder.  It can also be used as a fertilizer.  It is also a diuretic, although a poor one and humans should not use it.
1141237
depends if it is 25.9% nitrogen by molar weight or total # of atoms
219474
"Nitric acid 6.0"?  It sounds like something AOL would put out.\n\nNitric acid (HNO3) is a strong acid which is also quite reactive.  Nitric acid is used as a regagent in chemical reactions and in the production of many Nitrate compounds.\nI assume the "6.0" you are refering to may be its concentration?  6.0 Molar Nitric acid is quite concentrated and can do some real damage if you spill any or get any on your skin.  6.0 Molar means that in the acid, 6 Moles of HNO3 are dissolved in every 1 Liter of solution.  Nitric acid is a pretty "nasty" acid and geat care should be taken while using it.