Question

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

$$4\mathrm{Fe}(\mathrm{s})+3\mathrm{O}{\phantom{A}}_2(\mathrm{g})⟶2\mathrm{Fe}{\phantom{A}}_2\mathrm{O}{\phantom{A}}_3(\mathrm{g})$$

विकल्प

• Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore it follows law of conservation of mass.

• Total mass of reactants = total mass of product; therefore, law of multiple proportions is followed.

• Amount of $$\mathrm{Fe}{\phantom{A}}_2\mathrm{O}{\phantom{A}}_3$$ can be increased by taking any one of the reactants (iron or oxygen) in excess.

• Amount of $$\mathrm{Fe}{\phantom{A}}_2\mathrm{O}{\phantom{A}}_3$$ produced will decrease if the amount of any one of the reactants (iron or oxygen) is taken in excess.

Answer 1

Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore it follows law of conservation of mass.

Explanation:

$$4\mathrm{Fe}+3\mathrm{O}{\phantom{A}}_2⟶2\mathrm{Fe}{\phantom{A}}_2\mathrm{O}{\phantom{A}}_3$$ follows law of conservation of mass since mass of reactants is equal to mass of products.