Ferric oxide reacts with aluminium to produce aluminium oxide and iron. The balanced chemical equation for the given reaction is :
$F e_{2} O_{3}$ + $2 A l$ $\to$ $A l_{2} O_{3}$ + $2 F e$
Which of the following substances is oxidized in the given reaction?

Al2O3

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F e_{2} O_{3}

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Solution

The correct option is C Al
Al forms $A l_{2} O_{3}$ by the addition of oxygen. Hence, Al is getting oxidized.

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Similar questions

F e_{2} O_{3 (x)} F e r r i c o x i d e + 2 A l_{(x)} A l u m i n i u m \to A l_{2} O_{3 (x)} A l u m i n i u m o x i d e + 2 F e_{(x)} I r o n

Question 20.1

Write the balanced chemical equation for the following reaction and identify the type of reaction.

Thermit reaction: Iron (III) oxide reacts with aluminium and gives molten iron and aluminium oxide.

Translate the following statements into chemical equations and then balance the equations :

(a) Hydrogen sulphide gas burns in air to give water and sulphur dioxide.

(b) Phosphorus burns in oxygen to give phosphorus pentoxide.

(d) Aluminium metal replaces iron from ferric oxide, $F e_{2} O_{3}$ , giving aluminium oxide and iron.

(e) Barium chloride reacts with zinc sulphate to give zine chloride and barium sulphate.

1 m o l

(F e)

0.65 m o l O_{2}

F e O

F e_{2} O_{3}

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