c. If 3.50 g of phosgenite is produced in the laboratory from the amounts of starting materials stated in part (b), what is the percent yield of the reaction? Given, Experimental (actual) yield = 2.72 g
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Phosgenite, a lead compound with the formula $\mathrm{Pb}_{2} \mathrm{Cl}_{2} \mathrm{CO}_{3},$ is found in ancient Egyptian cosmetics. Phosgenite was prepared by the reaction of $\mathrm{Pb} \mathrm{O}, \mathrm{NaCl}$ $\mathrm{H}_{2} \mathrm{O},$ and $\mathrm{CO}_{2} .$ An unbalanced equation of the reaction is $\mathrm{PbO}(s)+\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(g) \rightarrow$.$$\mathrm{Pb}_{2} \mathrm{Cl}_{2} \mathrm{CO}_{3}(s)+\mathrm{NaOH}(a q)$$,a. Balance the equation. b. How many grams of phosgenite can be obtained from $10.0 \mathrm{g}$ of $\mathrm{PbO}$ and $10.0 \mathrm{g}$ of $\mathrm{NaCl}$ in the presence of excess water and $\mathrm{CO}_{2} ?$ c. If 2.72 g of phosgenite is produced in the laboratory from the amounts of starting materials stated in part (b), what is the percent yield of the reaction?
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