When FeCl3 is ignited in an atmosphere of pure oxygen, this reaction takes place:4FeCl3(s)+3O2(g)→2Fe2O3(s)+6Cl2(g) If 3 moles of FeCl3 are ignited in the presence of 2 moles of O2 gas, which of the following statements regarding to the given reaction is/are correct?

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When $F e C l_{3}$ is ignited in an atmosphere of pure oxygen, this reaction takes place:
$4 F e C l_{3} (s) + 3 O_{2} (g) \to 2 F e_{2} O_{3} (s) + 6 C l_{2} (g)$
If 3 moles of $F e C l_{3}$ are ignited in the presence of 2 moles of $O_{2}$ gas, which of the following statements regarding to the given reaction is/are correct?

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0.33 mole $F e C l_{3},$ remains unreacted

4 mole $C l_{2}$ is formed

1.33 moles of $F e_{2} O_{3}$ is formed

0.50 mole $O_{2}$ remains unreacted

answer is A, B, C.

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Detailed Solution

   $4 F e C l_{3 (s)} + 3 O_{2 (g)} \to 2 F e_{2} O_{3} + 6 C l_{2 (g)}$
Moles 3 2
Stoich amount    $\frac{3}{4}$    $\frac{2}{3}$
=0.75 0.67
L.R
A) $3 m o l O_{2} \to 4 m o l F e C l_{3}$
2    $\to ?$
   $= \frac{4}{3} \times 2$
   $= 2.67 r e a c t e d$
$∴$ unreacted =0.33 mol

B) $3 m o l O_{2} \to 6 m o l C l_{2}$
2    $\to ?$
$= \frac{6}{3} \times 2$
= 4 mol
C) $3 m o l O_{2} \to 2 m o l F e_{2} O_{3}$
2 $\to ?$
   $= \frac{2}{3} \times 2$
$= 1.33 m o l .$