Zinc is more active chemically than is silver; it can be used to remove ionic silver from solution.
Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s)
The concentration of a silver nitrate solution is determined to be 1.330 mol/L. Pieces of zinc totaling 100.0 g are
added to 1.000 L of the solution; 90.0 g of silver is collected.
a. Calculate the percent yield of silver.
b. Suggest a reason why the yield is less than 100.0%.

Question

Zinc is more active chemically than is silver; it can be used to remove ionic silver from solution.
Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s)
The concentration of a silver nitrate solution is determined to be 1.330 mol/L. Pieces of zinc totaling 100.0 g are 
added to 1.000 L of the solution; 90.0 g of silver is collected.
a. Calculate the percent yield of silver.
b. Suggest a reason why the yield is less than 100.0%.

cherylim23 · Answer

Determine which reactant is limiting and which is in excess. Calculate the expected mole to be collected for silver (i.e. expected yield) and hence the expected mass.
Take this answer, divide by 90.0 x 100% to get percentage yield.

There are many reasons why yield is 100%. If yield is more than 100%, it suggests that your silver collected is not pure. If yield is <100%, it could be possible that some silver is lost when filtering to obtain residue.

anonymous · Answer

Thanks. I should have known I was overcomplicating the problem.