Question

In Part 2 of this procedure, in the presence of oxygen, our Fe oxalate product will transform into \( \mathrm{Fe}_{2} \mathrm{O}_{3} \) with the release of \( \mathrm{CO}_{2} \) and \( \mathrm{H}_{2} \mathrm{O} \). In order to get the correct answers in our post-lab, we'll first need to balance these equations. Provide the stoichiometric coefficients to balance each. Use integer values. a. \( \square \) \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot \mathrm{H}_{2} \mathrm{O}(s)+ \) \( \square \) \( \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \) \( \square \) \( \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+ \) \( \square \) \( \mathrm{CO}_{2}(\mathrm{~g})+ \) \( \square \) \( \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \) b. \( \square \) \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})+ \) \( \square \) \( \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \) \( \square \) \( \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+ \) \( \square \) \( \mathrm{CO}_{2}(\mathrm{~g})+ \) \( \square \) \( \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \) c. \( \square \) \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot 3 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})+ \) \( \square \) \( \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \) \( \square \) \( \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+ \) \( \square \) \( \mathrm{CO}_{2}(\mathrm{~g})+ \) \( \square \) \( \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \)

          In Part 2 of this procedure, in the presence of oxygen, our Fe oxalate product will transform into \( \mathrm{Fe}_{2} \mathrm{O}_{3} \) with the release of \( \mathrm{CO}_{2} \) and \( \mathrm{H}_{2} \mathrm{O} \). In order to get the correct answers in our post-lab, we'll first need to balance these equations. Provide the stoichiometric coefficients to balance each. Use integer values.
a. \( \square \) \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot \mathrm{H}_{2} \mathrm{O}(s)+ \) \( \square \) \( \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \) \( \square \) \( \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+ \) \( \square \) \( \mathrm{CO}_{2}(\mathrm{~g})+ \)
\( \square \) \( \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \)
b. \( \square \) \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})+ \) \( \square \) \( \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \) \( \square \) \( \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+ \) \( \square \) \( \mathrm{CO}_{2}(\mathrm{~g})+ \) \( \square \) \( \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \)
c. \( \square \) \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot 3 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})+ \) \( \square \) \( \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \) \( \square \) \( \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+ \) \( \square \) \( \mathrm{CO}_{2}(\mathrm{~g})+ \)
\( \square \) \( \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \)

In Part 2 of this procedure, in the presence of oxygen, our Fe oxalate product will transform into Fe2O3 with the release of CO2 and H2O. In order to get the correct answers in our post-lab, we'll first need to balance these equations. Provide the stoichiometric coefficients to balance each. Use integer values.
a. □ FeC2O4·H2O(s)+ □ O2( g) → □ Fe2O3( s)+ □ CO2( g)+
□ H2O(g)
b. □ FeC2O4· 2 H2O(s)+ □ O2( g) → □ Fe2O3( s)+ □ CO2( g)+ □ H2O(g)
c. □ FeC2O4· 3 H2O(s)+ □ O2( g) → □ Fe2O3( s)+ □ CO2( g)+
□ H2O(g)

Added by Gregg M.

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