Zinc reacts with iodine in a synthesis reaction: $\mathrm{Zn}+\mathrm{I}_{2} \rightarrow \mathrm{Zn} \mathrm{l}_{2}$ a. Determine the theoretical yield if 1.912 mol of zinc is used. b. Determine the percent yield if 515.6 $\mathrm{g}$ of product is recovered.
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The balanced chemical equation shows that 1 mol of Zn reacts with 1 mol of I2 to produce 1 mol of ZnI2. Show more…
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Zinc reacts with iodine in a synthesis reaction: $\mathrm{Zn}+\mathrm{I}_{2} \rightarrow \mathrm{ZnI}_{2}$ \begin{equation} \begin{array}{l}{\text { a. Determine the theoretical yield if } 1.912 \text { mol of zinc is used. }} \\ {\text { b. Determine the percent yield if } 515.6 \mathrm{g} \text { of product is recovered. }}\end{array} \end{equation}
You determined the theoretical yield if 0.5 moles of zinc is used to form ZnI2. Determine the percent yield if 515.6 g of product is recovered. ___ Zn + __I2 → ___ZnI2
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Zinc sulfide reacts with oxygen according to the reaction: $$2 \mathrm{ZnS}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{ZnO}(s)+2 \mathrm{SO}_{2}(g) $$ A reaction mixture initially contains 4.2 $\mathrm{mol} \mathrm{ZnS}$ and 6.8 $\mathrm{mol} \mathrm{O}_{2}$ . Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
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