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Title: Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia.? Post by: buffnstuff on Mar 18, 2012 N2 (g) + 3H2 (g) --> 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.
Title: Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia.? Post by: julietalbot6 on Mar 18, 2012 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. |