The following is the balanced equation for the reaction in which ammonia (NH3) is used to produce the fertilizer ammonium nitrate: NH3+HNO3-->NH4NO3
A.
How many moles of NH3 are needed to make one mole of NH4NO3
B.
How many moles of HNO3 are needed to make one mole of NH4NO3
C.
Assume you have 51grams of NH3. Using the periodic tabl, compute the molar mass of NH3 and determine how many moles are present in the 51 grams.
D.
How many moles of NH4NO3 can be formed from the number of NH3 moles you got as your answer to(C)?
E.
Assume you have 63g of HNO3. Compute the molar mass of HNO3 and determine how many moles are present in the 63g.
F.
How many moles of NH4NO3 can be formed from the number of moles of HNO3 that you got as your answer for (E)
G.
How many moles of NH4NO3 can be formed from the given amounts of NH3 and HNO3?
H.
Which reactant is the limiting reactant, NH3 or HNO3
2006-10-26 07:13:00 · 5 answers · asked by cetinnovations 1 in Science & Mathematics ➔ Chemistry
Thank all of you for all your help!!!! I work so much that I scramble to just stay afloat
2006-10-26 07:52:16 · update #1
Your book should have a formula for converting into moles. It's very easy.
http://members.aol.com/profchm/mole.html
2006-10-26 07:27:53 · answer #1 · answered by Michael 4 · 0⤊ 0⤋
The stoichiometric ratios are all 1 (1 NH3 + 1 HNO3 -> 1 NH4NO3, if you want), so for A and B, the answers are 1: one mole of NH3 is used to make 1 mole of NH4NO3.
C: N's atomic weight is 14, H is 1, so NH3's molecular weight is 17 g/mol (14 + 1 * 3). 51 g / 17 g/mol = 3 mol NH3
D: 3 moles (again, it's a 1:1 ratio)
E: O's atomic weight is 16, os the molecular weight of HNO3 = 1 + 14 + 16*3 = 63 g/mol. 63 g / 63 g/mol = 1 mol HNO3.
F: 1 mol
G: you have 3 moles of NH3 and 1 mole of HNO3. The amount of NH4NO3 is limited to the smaller amount, so you can make 1 mol of NH4NO3
H: HNO3
2006-10-26 14:33:42 · answer #2 · answered by MadScientist 4 · 0⤊ 0⤋
damn boy i wish i could help but i cant remember a word about chemistry and equations since ive taken this subject last year and already 4got about it
guess ur gonna hv 2 do ur own work :P
2006-10-26 14:30:21 · answer #3 · answered by girl-witta-attitude 1 · 0⤊ 0⤋
If you just stopped wasting your time in internet, and just bothered to open your chemistry book, you'd know.
2006-10-26 14:21:20 · answer #4 · answered by The Potter Boy 3 · 0⤊ 0⤋
Damn, do your own homework...
2006-10-26 14:20:32 · answer #5 · answered by Pale 3 · 0⤊ 0⤋