Answer:
62.78%
Explanation:
2Pb + O2 —> 2PbO
To obtain the %yield, we must first obtain the theoretical yield. This can be achieved by doing the following:
Molar Mass of Pb = 207g/mol
Mass of Pb from the balanced equation = 2 x 207 = 414g
Molar Mass of PbO = 207 + 16 = 223g/mol
Mass of PbO from the balanced equation = 2 x 223 = 446g
From the equation,
414g of Pb reacted with O2 to produced 446g of PbO.
Therefore, 451.4g of Pb will react with O2 to produce =(451.4x446)/414 = 486.3g of PbO.
Therefore the theoretical yield of PbO is 486.3g.
Now we can obtain the the %yield as follows:
Actual yield = 305.3g
Theoretical yield = 486.3g
%yield =?
%yield = Actual yield/Theoretical yield x100
%yield = 305.3/486.3 x100
%yield = 62.78%
