Consider the reaction. 2 Pb ( s ) + O 2 ( g ) ⟶ 2 PbO ( s ) An excess of oxygen reacts with 451.4 g of lead, forming 367.5 g of lead(II) oxide. Calculate the percent yield of the reaction.

Answer : The percent yield of the reaction is, 75.6 %

Solution : Given,

Mass of Pb = 451.4 g

Molar mass of Pb = 207 g/mole

Molar mass of PbO = 223 g/mole

First we have to calculate the moles of Pb.

Now we have to calculate the moles of

The balanced chemical reaction is,

From the reaction, we conclude that

As, 2 mole of react to give 2 mole of

So, 2.18 mole of react to give 2.18 mole of

Now we have to calculate the mass of

Theoretical yield of = 486.1 g

Experimental yield of = 367.5 g

Now we have to calculate the percent yield of the reaction.

Therefore, the percent yield of the reaction is, 75.6 %

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.