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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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meerkat18
Given the reaction 2Pb(s)+O2(g)= 2PbO(s) and a reactant amount of 451.4 grams, we are asked for the yield of the reaction. The amount of lead present produces 451.4/207.2 *( 2/2) *(223.2) via 100% conversion, 486.26 grams lead (II) oxide. hence the percent yield is 356.7g /486.26 g or equal to 73.35 percent

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