Number of electrons (x) involved in the following reaction is :
\(N \equiv N+ 8H^{+}+x \rightarrow 2N H^{3}+ H_{2}\)
Nitrogen Reaction Electron Transfer Analysis
The question asks us to determine the number of electrons, represented by 'x', involved in the following chemical reaction:
$ N \equiv N + 8H^{+} + x \rightarrow 2NH^{3} + H_{2} $
This reaction involves a change in the oxidation state of nitrogen, indicating a redox process. To find 'x', we need to analyze the oxidation states of nitrogen before and after the reaction.
Nitrogen Oxidation State Analysis
Initial Oxidation State of Nitrogen:
In the reactant side, we have diatomic nitrogen, \( N \equiv N \). In its elemental form, the oxidation state of nitrogen is 0.
Final Oxidation State of Nitrogen:
On the product side, nitrogen is present in ammonia, \( NH^3 \). In ammonia, hydrogen typically has an oxidation state of +1. Let the oxidation state of nitrogen be \( N_{ox} \).
$ N_{ox} + 3 \times (+1) = 0 $
Solving for \( N_{ox} \):
$ N_{ox} = -3 $
So, the oxidation state of nitrogen in \( NH^3 \) is -3.
Calculating Electrons Transferred (x)
The reaction shows \( N \equiv N \) converting to \( 2NH^3 \). This means we are looking at the transformation of one molecule of \( N_2 \) into two molecules of \( NH_3 \).
The change in oxidation state for one nitrogen atom is from 0 to -3. This represents a gain of 3 electrons per nitrogen atom.
$ N(0) \rightarrow N(-3) \quad (\text{Gain of } 3e^-) $
Since the reactant molecule is \( N_2 \) (containing two nitrogen atoms), and it forms \( 2NH_3 \) (also containing two nitrogen atoms in total), the total number of electrons gained during this reduction process is:
$ \text{Total electrons gained} = (\text{Number of N atoms}) \times (\text{Electrons gained per N atom}) $
$ \text{Total electrons gained} = 2 \times 3 $
$ \text{Total electrons gained} = 6 $
The variable 'x' in the reaction equation represents the total number of electrons transferred. Therefore, \( x = 6 \).
Conclusion
The number of electrons involved in the reduction of \( N_2 \) to \( NH_3 \) in this reaction is 6. Thus, \( x = 6 \).
Checking the Options:
- Option 1: 8
- Option 2: 6
- Option 3: 4
- Option 4: 10
Based on our calculation, the correct value for 'x' is 6.
Important Questions from Redox Reactions
Nitric acid is reduced to nitrogen dioxide in which of the following reactions?
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In reaction, 2Na2S2O3 + I2 → A + 2NaI; A will be _________.
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- In the following redox reaction, which compound is acting as a reducing agent ?
\(N_2H_4 + 2H_2O_2 \rightarrow N_2 + 4H_2O\)
