In the following reaction, 451.4g of lead reacts with excess oxygen forming 356.7g of lead (II) oxide. Calculate the percent yield of the reaction. 2Pb (s) + O2 (g) = 2PbO (s)

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Chemistry

24 February, 03:46

In the following reaction, 451.4g of lead reacts with excess oxygen forming 356.7g of lead (II) oxide. Calculate the percent yield of the reaction. 2Pb (s) + O2 (g) = 2PbO (s)

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William Obrien · Answer 1

The stoichoimetric ratio of lead to lead oxide is 2:2. Given 451.4 grams of lead, we get the moles multiply by 2/2 or 1 and the molar mass of lead oxide, we get a product of 486.26 g lead oxide. The percent yield is the actual amount, 356.7 grams over 486.26 grams which is equal to 73.36% yield.