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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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buffnstuff buffnstuff
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12 years ago
N2 (g) + 3H2 (g) Rightwards Arrow 2NH3 (g)    If the reaction yield is 87.5%, how many moles of N2 are needed to produce 3.00 mol NH3? Could someone please show me how to solve this step by step.  Only 2 people in our chem class passed our exam over this stuff.... needless to say I wasn't one of them.
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#1
12 years ago
If the yield was 100%, by the balanced equation you would need 1.5 moles N2 to produce 3 moles NH3 - the ratio is 1:2. Hopefully that part is easy enough.

With a yield of 87.5% you would need more N2, increased by a ratio of 100/87.5. That's more common sense than anything else. So the final answer would be

100/87.5 * 1.5 =  1.7 moles N2.
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