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ShopStylista: Terms & Conditions

Audrey

Mon, 09 Nov 2009 10:45:00 GM

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What is the theoretical yield for this reaction under the given conditions?
Q. 1.93 g H_2 is allowed to react with 9.81 g N_2, producing 1.55 g NH_3. 3H_2(g) + N_2(g) ---> 2NH_3(g) A)What is the theoretical yield for this reaction under the given conditions? B) What is the percent yield for this reaction under the given conditions? Thanks guys please explain how to do if you can, thank you!
Asked by Vincent M - Wed Oct 15 03:51:27 2008 - - 1 Answers - 1 Comments

A. Your requirements are 3 moles H2 to 1 mole N2 to yield 2 moles of NH3 1.93 g H2 = 0.965 moles H2 9.81 g N2 = 0.350 moles N2 1.55 g NH3 = 0.0912 moles NH3 The ratio of H2 to N2 is 2.76, but you need 3, so there is not enough H2; H2 is the limiting reagent and will determine the amount of NH3 produced. Each mole of H2 yields 2/3 moles of NH3, so you should get 0.965*(2/3) = 0.643 moles (10.9 g) of NH3, and that is the theoretical yield. The actual yield is 0.0912 moles, so the percent yield is 0.0912/0.643 * 100 = 14.2%
Answered by gp4rts - Wed Oct 15 04:18:22 2008