Answer to Question #135322 in General Chemistry for Izzy Deliman

Question #135322
5. The Haber- process has been the primary method for the Industrial production of ammonia (NH 3 ) for over 100 years N 2 (q)+3H 2 (q) 2NH 3 lg) mass of ammonia can be produced by 7.19 * 10 ^ 9 * q of nitrogen gas and 1.19 * 10 ^ 9 / g of hydrogen gas ?
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Expert's answer
2020-09-29T06:48:07-0400

N2(g)+3H2(g)    2NH3(g)N _2 (g)+3H _2 (g) \implies2NH _3 (g)


moles of Nitrogen here =7.19×10928=2.56×108\frac{7.19\times10^9}{28}=2.56\times10^8


moles of Hydrogen here =1.19×1092=5.95×108\frac{1.19\times10^9}{2}=5.95\times10^8


here for every mole of nitrogen 3 moles of hydrogen is required and 2 moles of ammonia is formed

clearly from the above mole quantities we can see that hydrogen is the limiting reagent here


x=5.95×1083=1.98×108x=\frac{5.95\times10^8}{3}=1.98\times10^8

moles of ammonia formed =2x=2×1.98×108=3.96×1082x=2\times1.98\times10^8=3.96\times10^8

mass of ammonia formed =17×3.96×108=6.73×109grams17\times3.96\times10^8=6.73\times10^9 grams


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