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5) For the reaction 2NO+ 0, 2NO, 10 grams of NO are mixed with 7 grams of O, A) What is the limiting reagent? B) What is the theoretical yield of NO,? -C) If the actual yield of NO2 is 9 grams, what is the percent yield of the reaction?
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Answer 5 Reaction involved MW of nitric oxide (NO) = 30 MW of oxygen (O2)-16 MW of nitrogen dioxide NO)-46 Here, 2 mole of NO react with 1 mole O2 to produce 2 mole of NO2 or, 2 x 30-60 g ofNO react with 16 g of O2 to produce 2 x 46-92 g 0fN02 When 10 g of NO are mixed with 7 g of O2 , then, NO will act as limiting reagent means NO will be fully consumed after the reaction. Therefore, 10 g of NO will react with (10 x 16) 60 2.67 g of O2 , to produce (10 x92) /60 15.33 g of NO Therefore, here theoritical yield of NO2-15.33 g NO2 If actual yield of NO29 g NO2 Then, percentage yield-Actual yield /theoritical yield) x 100 9/15.33) x 100 58.71 %

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