Chemistry · Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number and balancing of redox reactions
In the reaction, the change of to involves:
In the reaction, \( \mathbf{3} \boldsymbol{C u} \boldsymbol{O}+\mathbf{2 N H}_{3} \longrightarrow \boldsymbol{N}_{2}+\mathbf{3} \boldsymbol{H}_{2} \boldsymbol{O}+ \) \( \mathbf{3} C u \) the change of \( N H_{3} \) to \( N_{2} \) involves:
- A. Loss of 6 electrons per mole of \( N_{2} \)
- B. Loss of 3 electrons per mole of \( N_{2} \)
- C. Gain of 6 electrons per mole of \( N_{2} \)
- D. Gain of 3 electrons per mole of \( N_{2} \)
Step-by-step solution
In NH3, nitrogen has oxidation state -3. In N2, each nitrogen has oxidation state 0. Each nitrogen atom loses 3 electrons, and since N2 contains two nitrogen atoms, total loss is 6 electrons per mole of N2.
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