# Problem: A 27.6-mL sample of a 1.62 M potassium chloride solution is mixed with 14.6 mL of a 0.890 M lead(II) nitrate solution and this precipitation reaction occurs:2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)The solid PbCl2 is collected, dried, and found to have a mass of 2.56 g. Determine the limiting reactant, the theoretical yield, and the percent yield.Determine the percent yield.

###### FREE Expert Solution

Recall molarity (M):

2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)

Calculate the mass of PbCl2 produced from each reactant:

PbCl2 from KCl

molar mass PbCl2 = 278.1 g/mol

mass PbCl2 = 6.21 g

PbCl2 from Pb(NO3)2

molar mass PbCl2 = 278.1 g/mol

80% (53 ratings) ###### Problem Details
A 27.6-mL sample of a 1.62 M potassium chloride solution is mixed with 14.6 mL of a 0.890 M lead(II) nitrate solution and this precipitation reaction occurs:

2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)

The solid PbCl2 is collected, dried, and found to have a mass of 2.56 g. Determine the limiting reactant, the theoretical yield, and the percent yield.

Determine the percent yield.