A58.0ml sample of a 0.122m potassium sulfate solution is mixed with 40.0ml of a 0.102m lead(ii) acetate solution and this precipitation reaction occurs:

k2so4(aq)+pb(c2h3o2)2(aq)→2kc2h3o2( aq)+pbso4(s)

the solid, pbso4, is collected, dried, and found to have a mass of 0.993g.

determine the:

1) limiting reactant
2) theoretical yield
3) percent yield

1) Limiting reactant: Pb(C2H3O2)2

2) Theoretical Yield: 1,237 gr

3) Percent Yield: 80,27%

Explanation:

The limiting reactant is the reactant that is consumed first in the reaction. We find it by dividing the amount of moles of each reagent by its molar coefficient in the balanced reaction, the lowest value corresponds to the limiting reagent.

The theoretical yield is how much product is produced using the limiting reactant as the starting point.

The percent yield is the fraction between the real products obtained and the theoretical yield, all multiplied by 100.

K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s)

Limiting reactant:

The equation is already balanced, now we find the moles of each reactant and divide it by their molar coefficient:

K2SO4 (molar coefficient=1):

Pb(C2H3O2)2 (molar coefficient=1):

As 0,00408 is lower than 0,00708, Pb(C2H3O2)2 is the limiting reactant.

Theoretical yield:

Now we find the amount of PbSO4 produced starting from the limiting reactant.

Percent yield:

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