Question

(a)Translate the following statements into balanced chemical equation. Hydrogen gas combines with nitrogen to form ammonia. (b) Identify the oxidised and reduced substance in the given reaction. 3Fe + 4H20 → Fe304 + 4H2​

Answer 1

$\Large{\underline{\underline{\red{\tt{\purple{\leadsto } SolutioN:-}}}}}$

$\tt\green{ Given\:questions\: are:-}$

• Translate the following statements into balanced chemical equation. Hydrogen gas combines with nitrogen to form ammonia.
• Identify the oxidised and reduced substance in the given reaction 3Fe + 4H20 $\longrightarrow$Fe304 + 4H2.

$\blue{\bf Ans\:a)}$ We know that Hydrogen gas reacts with Nitrogen to form ammonia .

Symbols of atoms in this reacⁿ are ,

• $\sf Hydrogen - H_2$
• $\sf Nitrogen - N_2$
• $\sf Ammonia - NH_3$

$\pink{\bf \mapsto The \:skeletal\: equation \:would\: be:}$

$\boxed{\red{\bf\blue{ \leadsto} \underset{\blue{Hydrogen}}{H_2}\:+\:\underset{\blue{Nitrogen}}{N_2}\:\longrightarrow \:\underset{\blue{Ammonia}}{NH_3}}}$

Now here number of atoms on LHS and RHS is :

$\boxed{\begin{tabular}{|c|c|c|}\cline{1-3}\bf Atoms &\bf LHS&\bf RHS\\\cline{1-3} Hydrogen & 2&3\\\cline{1-3} Nitrogen&2&1 \\\cline{1-3}\end{tabular}}$

Here number of atoms on LHS and RHS is not same so the equation isn't balanced . So , after balancing the equation becomes ,

$\boxed{\red{\bf\blue{ \leadsto} \underset{\blue{Hydrogen}}{3H_2}\:+\:\underset{\blue{Nitrogen}}{N_2}\:\longrightarrow \:\underset{\blue{Ammonia}}{2NH_3}}}$

Now here number of atoms on LHS and RHS is :

$\boxed{\begin{tabular}{|c|c|c|}\cline{1-3}\bf Atoms &\bf LHS&\bf RHS\\\cline{1-3} Hydrogen & 2\times3=6 & 3\times2=6 \\\cline{1-3} Nitrogen&2& 2\times1=2 \\\cline{1-3}\end{tabular}}$

Here number of atoms on LHS and RHS is same so the equation is now balanced .

_________________________________

$\blue{\bf Ans\:b)}$ Firstly we must know what oxidation and reduction are .

$\underline{\green{\bf \dag OxidatioN:-}}$

Addition of oxygen aur electronegative element to a substance or removal of hydrogen is called oxidation.

$\underline{\green{\bf \dag ReductioN:-}}$

Addition of Hydrogen or electropositive element to a substance or removal of oxygen of electronegative substance is called reduction.

$\underline{\green{\bf \dag RedoX\:ReactioN:-}}$

A reaction in which loss and gain of electron take place simultaneously is called a Redox reaction.

$\tt Now \:here\:the\:given\:reaction\:is$

$\boxed{\red{\bf\blue{ \leadsto} \underset{\blue{Iron}}{3Fe}\:+\:\underset{\blue{Water}}{4H_2O}\:\longrightarrow \:\underset{\blue{Iron(III)oxide}}{Fe_3O_4}}}$

As per definition we know addition of oxygen is called oxidation or removal of hydrogen is called oxidation and adoption of hydrogen or removal of oxygen is called reduction .

So , here in this reaction Oxygen is added to Iron so it is oxidized and oxygen is removed from Hydrogen so it is reduced .Also here Water is oxidising agent .