215. For the reaction: $\text{PH}_3(\text{g}) + \text{O}_2(\text{g}) \rightarrow \text{P}_4\text{O}_{10}(\text{s}) + \text{H}_2\text{O}(\text{l})$, after balancing, what is the difference between the sum of the stoichiometric coefficients of the reactants and the sum of the stoichiometric coefficients of the products? If the percent yield of this reaction is 85\%, and 1/6 mol $\text{PH}_3$ is consumed, how many moles of $\text{P}_4\text{O}_{10}$ are obtained? (1) displacement: 4, reduction: 0/64 (2) oxidation -- reduction: 5, 0/64 (3) displacement: 5, reduction: 0/34 (4) oxidation -- reduction: 4, 0/34
\textbf{215.} For the reaction: $\text{PH}_3(\text{g}) + \text{O}_2(\text{g}) \rightarrow \text{P}_4\text{O}_{10}(\text{s}) + \text{H}_2\text{O}(\text{l})$, after balancing, what is the difference between the sum of the stoichiometric coefficients of the reactants and the sum of the stoichiometric coefficients of the products? If the percent yield of this reaction is 85\%, and 1/6 mol $\text{PH}_3$ is consumed, how many moles of $\text{P}_4\text{O}_{10}$ are obtained?
\begin{center}
(1) displacement: 4, reduction: 0/64 \qquad (2) oxidation -- reduction: 5, 0/64 \\
(3) displacement: 5, reduction: 0/34 \qquad (4) oxidation -- reduction: 4, 0/34
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