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Stoichiometry \( \mid 5-13 \) Stoichiometry: Postlab Questions \( \qquad \) Name \( \qquad \) \( \frac{1411 / 5 L}{\text { Section }} \) \( \qquad \) PrVillanueva TA 1. \( \mathrm{Fe}(\mathrm{OH})_{3} \), the product in today's reaction, is actually unstable in water, and decomposes to \( \mathrm{Fe}_{2} \mathrm{O}_{3} \). \[ 2 \mathrm{Fe}(\mathrm{OH})_{3} \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}+3 \mathrm{H}_{2} \mathrm{O} \] a. Would this decomposition reaction change the limiting reactant and excess reactant? No the decomposition veaction doesn't ouneng the limiting or original ferm b. Using your data (mass of limiting reactant), what is the theoretical yield if all the product \( \mathrm{Fe}(\mathrm{OH})_{3} \) decomposed to \( \mathrm{Fe}_{2} \mathrm{O}_{3} \) ? \[ \begin{array}{l} F_{e}(\mathrm{OH})_{3}=106.87 \mathrm{~g} / \text { mol } \\ \mathrm{Fe}_{2} 03=159.70 \mathrm{~g} \text { gimol } \\ \text { Theovetical yide }=\text { moles of } \mathrm{Fe}_{2} 03 \times 159.7 \end{array} \] c. If the mass of your precipitate (Part I, blank \#6) is actually the mass of \( \mathrm{Fe}_{2} \mathrm{O}_{3} \), what is your percent yield?

          Stoichiometry \( \mid 5-13 \)

Stoichiometry: Postlab Questions
\( \qquad \)
Name \( \qquad \)
\( \frac{1411 / 5 L}{\text { Section }} \) \( \qquad \)
PrVillanueva TA
1. \( \mathrm{Fe}(\mathrm{OH})_{3} \), the product in today's reaction, is actually unstable in water, and decomposes to \( \mathrm{Fe}_{2} \mathrm{O}_{3} \).
\[
2 \mathrm{Fe}(\mathrm{OH})_{3} \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}+3 \mathrm{H}_{2} \mathrm{O}
\]
a. Would this decomposition reaction change the limiting reactant and excess reactant?
No the decomposition veaction doesn't ouneng the limiting or
original ferm
b. Using your data (mass of limiting reactant), what is the theoretical yield if all the product \( \mathrm{Fe}(\mathrm{OH})_{3} \) decomposed to \( \mathrm{Fe}_{2} \mathrm{O}_{3} \) ?
\[
\begin{array}{l}
F_{e}(\mathrm{OH})_{3}=106.87 \mathrm{~g} / \text { mol } \\
\mathrm{Fe}_{2} 03=159.70 \mathrm{~g} \text { gimol } \\
\text { Theovetical yide }=\text { moles of } \mathrm{Fe}_{2} 03 \times 159.7
\end{array}
\]
c. If the mass of your precipitate (Part I, blank \#6) is actually the mass of \( \mathrm{Fe}_{2} \mathrm{O}_{3} \), what is your percent yield?

Stoichiometry | 5-13

Stoichiometry: Postlab Questions

Name
(1411 / 5 L)/( Section )
PrVillanueva TA
1. Fe(OH)3, the product in today's reaction, is actually unstable in water, and decomposes to Fe2O3.

2 Fe(OH)3→Fe2O3+3 H2O

a. Would this decomposition reaction change the limiting reactant and excess reactant?
No the decomposition veaction doesn't ouneng the limiting or
original ferm
b. Using your data (mass of limiting reactant), what is the theoretical yield if all the product Fe(OH)3 decomposed to Fe2O3 ?

Fe(OH)3=106.87 g / mol
Fe2 03=159.70 g gimol
Theovetical yide = moles of Fe2 03 × 159.7

c. If the mass of your precipitate (Part I, blank #6) is actually the mass of Fe2O3, what is your percent yield?

Added by Shaun W.

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