Given balanced reaction is 2Pb(s) + O2(g) ----> 2PbO(s)
Molar mass (g/mole) 207.2 32 223.2
From the above balanced reaction,
2 moles = 2*207.2g = 414.4 g of Pb reacts with excess of O2 produces 2 moles = 2*223.2g = 446.4 g of PbO
451.4g of Pb reacts with excess of O2 produces M g of PbO
M = ( 451.4g*446.4g) / 414.4g
= 486.3 g
This is the theoretical yield(486.3g)
But given that the actual yield is 319.3g
So percentage yield = ( actual yield/theoretical yield)*100
= ( 319.3g/486.3g) *100
= 65.7 %
Therefore the percentage yield is 65.7%
Assignment Score: 233/2000 Resources Hint Check Answer Question 16 of 20 Consider the reaction 2 Pb(s)...
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