The reaction of 9.66 g O2 with 9.33 g NO produces 10.1 g NO2. What is the percen

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Okay, to calculate the percent yield you first must balance the equation. 2NO+ O2 --> 2NO2 you add a 2 coefficient to NO2 to balance the number of nitrogens and oxygens. You next must find the theoretical yield-the most grams of NO2 that could possibly be produced by this reaction. You convert the grams of NO to moles of NO and moles of NO2 to grams of NO2. NO is the limiting reactant as it requires 2 moles of NO2 to make one mole of NO2. 9.66g NO * 1 mol NO/(14g +16 g) * 1 mol NO2/2 mol NO * 46 g NO2/ 1 mol NO2 = 7.406 g NO2 This number is the maximum number of grams of NO2 that can be produced by the reaction. Divide the actual yield by the theoretical yield and multiply by 100 to get the percent yield. (7.406 g NO2/ 10.1 g N02) * 100% = 73.3 % yield and the answer will be written as 73% yield to keep the same number of significant figures.

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