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13. Which of the following statements is correct about the reaction given below:

[tex]\[
4 \text{Fe} (s) + 3 \text{O}_2 (g) \longrightarrow 2 \text{Fe}_2 \text{O}_3 (s)
\][/tex]

(i) Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product; therefore, it follows the law of conservation of mass.

(ii) Total mass of reactants = total mass of product; therefore, the law of multiple proportions is followed.

(iii) The amount of [tex]\(\text{Fe}_2 \text{O}_3\)[/tex] can be increased by taking any one of the reactants (iron or oxygen) in excess.

(iv) The amount of [tex]\(\text{Fe}_2 \text{O}_3\)[/tex] produced will decrease if the amount of any one of the reactants (iron or oxygen) is taken in excess.

Sagot :

GinnyAnsweridn
Let's analyze each statement concerning the given reaction:

[tex]\[ 4 \, \text{Fe (s)} + 3 \, \text{O}_2 \, \text{(g)} \longrightarrow 2 \, \text{Fe}_2\text{O}_3 \, \text{(g)} \][/tex]

1. Statement (i): Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product; therefore it follows the law of conservation of mass.
- Explanation: The law of conservation of mass states that in a chemical reaction, the mass of the reactants must equal the mass of the products. The reaction shows that 4 moles of Iron (Fe) combine with 3 moles of Oxygen (O₂) to form 2 moles of Iron (III) Oxide (Fe₂O₃). This balancing of moles confirms that the total mass of the reactants equals the total mass of the products. This statement is True.

2. Statement (ii): Total mass of reactants = total mass of product; therefore, law of multiple proportions is followed.
- Explanation: The law of multiple proportions is different from the law of conservation of mass. It states that when elements combine, they do so in the ratio of small whole numbers. The context of this statement does not correctly apply to the law of multiple proportions but rather describes the law of conservation of mass again. However, as it's focusing on mass equality, this explanation is True implying the total mass of reactants equals the total mass of the product.

3. Statement (iii): Amount of Fe₂O₃ can be increased by taking any one of the reactants (iron or oxygen) in excess.
- Explanation: In a chemical reaction, increasing the quantity of one reactant (while keeping others available) can lead to an increased amount of product, provided that it is not a limiting reagent scenario. Thus, taking more iron or oxygen can indeed increase the amount of Fe₂O₃ produced. This statement is True.

4. Statement (iv): Amount of Fe₂O₃ produced will decrease if the amount of any one of the reactants (iron or oxygen) is taken in excess.
- Explanation: Taking one reactant in excess does not decrease the amount of product. Instead, it should either have no effect (if the other reagent is the limiting factor already) or increase the amount of the product, as explained in (iii). Therefore, this statement is False.

Thus, based on this detailed step-by-step analysis, the correct evaluations of the statements are:

- Statement (i): True
- Statement (ii): True
- Statement (iii): True
- Statement (iv): False
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