Chapter 9, Problem 91AP

Interpretation Introduction

(a)

Interpretation:

The number of moles of KCl produced with 3.50 moles of ${\text{P}}_{\text{2}}{\text{O}}_{\text{5}}$ should be determined.

Concept Introduction:

The reaction for lighting a match is as follows:

  $3{\text{P}}_{\text{4}}\left(s\right)+10{\text{KClO}}_{\text{3}}\left(s\right)\stackrel{\text{heat}}{\to }10\text{KCl}\left(s\right)+6{\text{P}}_{\text{2}}{\text{O}}_{\text{5}}\left(s\right)$

From the above reaction, 3 moles of ${\text{P}}_{\text{4}}$ reacts with 10 moles of ${\text{KClO}}_{\text{3}}$ to give 10 moles of KCl and 6 moles of ${\text{P}}_{\text{2}}{\text{O}}_{\text{5}}$.

Thus, number of moles of KCl can be calculated by comparing it with number of moles of ${\text{P}}_{\text{2}}{\text{O}}_{\text{5}}$ according to balanced chemical reaction.

Interpretation Introduction

(b)

Interpretation:

Number of moles of ${\text{P}}_{\text{4}}$ produces from 3.50 moles of ${\text{P}}_{\text{2}}{\text{O}}_{\text{5}}$ in the reaction should be calculated.

Concept Introduction:

From the above reaction, 3 moles of ${\text{P}}_{\text{4}}$ reacts with 10 moles of ${\text{KClO}}_{\text{3}}$ to give 10 moles of KCl and 6 moles of ${\text{P}}_{\text{2}}{\text{O}}_{\text{5}}$.

Thus, number of moles of ${\text{P}}_{\text{4}}$ can be calculated by comparing it with number of moles of ${\text{P}}_{\text{2}}{\text{O}}_{\text{5}}$ according to balanced chemical reaction.