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Chapter 9: Problem 34
Reacting 991 mol of \(\mathrm{SiO}_{2}\) with excess carbon yields 30.0 \(\mathrm{kg}\) of \(\mathrm{SiC.}\) What is the percentage yield? $$\mathrm{SiO}_{2}+3 \mathrm{C} \rightarrow \mathrm{SiC}+2 \mathrm{CO}$$
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What are three areas of a car's operation or design that depend on stoichiometry?
Use the balanced equation below to write mole ratios for the situations that follow. $$2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)$$ \begin{equation}\begin{array}{l}{\text { a. calculating mol } \mathrm{H}_{2} \mathrm{O} \text { given mol } \mathrm{H}_{2}} \\ {\text { b. calculating mol } \mathrm{O}_{2} \text { given mol } \mathrm{H}_{2} \mathrm{O}} \\ {\text { c. calculating mol } \mathrm{H}_{2} \text { given mol } \mathrm{O}_{2}}\end{array}\end{equation}
Design an experiment to measure the percentage yields for the reactions listed below. If your teacher approves your design, get the necessary materials, and carry out your plan. a. \(\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)\) b. \(2 \mathrm{NaHCO}_{3}(s) \longrightarrow\) $$ \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}_{2}(g) $$ c. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow\) $$ \mathrm{CaCO}_{3}(s)+2 \mathrm{NaCl}(a q) $$ d. \(\mathrm{NaOH}(a q)+\mathrm{HCl}(a q) \longrightarrow\) $$ \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$
Nitrogen dioxide from exhaust reacts with oxygen to form ozone. What mass of ozone could be formed from 4.55 \(\mathrm{g} \mathrm{NO}_{2} ?\) If only 4.58 \(\mathrm{g} \mathrm{O}_{3}\) formed, what is the percentage yield? $$\mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{O}_{3}(g)$$
How many liters \(\mathrm{N}_{2},\) density \(0.92 \mathrm{g} / \mathrm{L},\) can be made by the decomposition of 2.05 \(\mathrm{g} \mathrm{NaN}_{3} ?\) $$2 \mathrm{NaN}_{3}(s) \rightarrow 2 \mathrm{Na}(s)+3 \mathrm{N}_{2}(g)$$
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