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posted by  kk35 on 2/22/2008 6:52:45 PM  |  status: Live  

Haber process

Course Textbook Chapter Problem
Organic Chemistry Hein handout N/A
Question Details:
The Haber process for ammonia production is given by the balanced reaction:
N2(g) + 3H2(g)-----> 2NH3(g).  How many grams of each reactant would be required to produce 9.4 moles of product?  Must show work.
 
 
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posted by Clark on 2/22/2008 7:38:35 PM  |  status: Live
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Response Details:
Since you have moles of NH3, you have to convert moles of that to moles of each reactant.  Therefore:
9.4 moles NH3 x 3 moles H2 / 2 moles NH3 = 14.1 moles of H2
9.4 moles NH3 x 1 mole N2 / 2 moles NH3 = 4.7 moles of N2
 
Now that you have the moles of each reactant, all you have to do is convert from moles of each reactant to grams by finding the molar mass of nitrogen gas and hydrogen gas:
14.1 moles H2 x 2(1.00795)g / 1 mol H2 = 28.42g of H2
4.7 moles of N2 x 2(14.00674) / 1 mol N2 = 131.66g of N2
 
∴ you have 131.66g of N2 and 28.42g of H2.  I hope this helps!!
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