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Title: theoretical yield Post by: sashahobson on Feb 23, 2014 Elemental S reacts with O2 to form SO3 according to the reaction
2S+3O2→2SO3 A.) How many O2 molecules are needed to react with 5.59g of S? =1.57×10^23 molecules B.) What is the theoretical yield of SO3 produced by the quantities described in Part A? Can someone explain part B to me? Thank you. Title: Re: theoretical yield Post by: padre on Feb 23, 2014 HI
Here is a similar question, just switch the numbers and do the calculations over again Question Elemental S reacts with O2 to form SO3 according to the reaction 2S+3O2 -> 2SO3 1) How many O2 molecules are needed to react with 6.18 g of S? 2)What is the theoretical yield of SO3 produced by the quantities described in Part 1? Solution 1. convert to moles of sulfur 6.18g sulfur * ( 1 mol sulfur/32.065 g sulfur) = 0.1927 mol sulfur 2. find out how many moles of O2 needed use conversion factors ( For two moles of sulfur, you need three moles of oxygen) and (1 mol equal to 6.022x10^23) 0.1927 mol sulfur x (3 mol O2/ 2 mol S) = 0.2890 mol of O2 x (6.022x10^ 23 molecules of O2/mol O2) 1.74*10^23 molecules of O2 3. Theo yield: use the either moles of O2 or moles of S to find the ratio. The easiest to use in this case is S because 2 moles of S produces 2 moles of SO3 so..... 0.1927 mol sulfur = 0.1927 moles of SO3 use conversion factor (80.06 g/mol for sulfur trioxide) 0.1927 mol sulfur x (80.06 g/mol of SO3) = 15.4 g SO3 Title: Re: theoretical yield Post by: P-Chem? on Mar 3, 2014 percent yield = actual yield/theoretical yield x 100
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