CHEM 1031 Lecture Notes - Lecture 8: Molar Mass, Limiting Reagent, Ammonia

• School: Temple University
• Department: Chemistry
• Course: CHEM 1031
• Professor: John B.Michel

Document Summary

If a is a(cid:374) (cid:862)lr(cid:863), the(cid:374) b is i(cid:374) e(cid:454)(cid:272)ess (cid:862)inx (cid:863: ex. 2 c4h10 + 13 o2 > 8 co2 + 10 h2o. Nh3: grams n2 (31. 5) x 1 mole n2/ 28. 02 n2 x 2 moles nh3/ 1 mole n2 = 2. 25 mol. Nh3: lr: h2, inxs: n2, maximum yield = 1. 77 mole nh3 x 17. 03 g nh3/ 1 mol = 29. 3 g nh2. In most chemical reactions, the theoretical yield does not equal the actual yield. You always produce fewer grams of product than predicted. Due to impurities, some product being washed away when purified, or there could be side reactions occurring: % yield = actual (experimental) yield/ theoretical (maximum) yield x 100, ex. In previous example, the actual yield was 25. 2 g nh3, so percent yield will be actual yield (25. 2 g) divided by the theoretical yield (29. 3 g nh3) x 100= 86. 0% (pretty good: ex.