Question

Ancient Egyptians used several lead compounds as pigments in cosmetics and suffered from lead poisoning. one such pigment was PbClOH. It can be prepared bu the reactions below

PbO + NaCl + H2O ---> PbClOH + NaOH You start with 250 g o PbO and 50 g of NaCl, and excess H₂O. If you get 200 g of PbClOH product, what is the precent yield
a.) 100%
b.) 82%
c.) 73%
d.) 91%

Answer 1

Using the given masses of PbO and NaCl, along with the actual yield of PbClOH, the percent yield is calculated to be approximately 64.23%, which does not match any of the provided answer choices.

Step-by-step explanation:

To calculate the percent yield, we first need to compare the actual yield to the theoretical yield of PbClOH. The theoretical yield is the amount of product that would be obtained if the reaction were perfect. We can calculate the theoretical yield by using the stoichiometry of the balanced chemical equation and the initial masses of the reactants. However, we are only given the actual yield, which is 200 g of PbClOH.

Assuming that PbO was the limiting reagent, we can calculate the moles of PbO, which is 250 g / 223.2 g/mol = 1.12 mol (since the molar mass of PbO is 223.2 g/mol). According to the balanced equation, 1 mol of PbO yields 1 mol of PbClOH, hence, the theoretical yield is 1.12 mol x 278.1 g/mol (molar mass of PbClOH) = 311.472 g. The percent yield is then calculated by the formula:

Percent Yield = (Actual Yield/Theoretical Yield) x 100%

In this case, the calculation is:

Percent Yield = (200 g / 311.472 g) x 100% ≈ 64.23%

However, because none of the answer choices given match this result (there appears to be a discrepancy in the actual yield), we must acknowledge that the correct percent yield is not presented in the given options. Therefore, none of the listed answer choices (a, b, c, d) are correct.