Question

Problem page write a balanced half-reaction for the reduction of gaseous nitrogen n2 to aqueous hydrazine n2h4 in acidic aqueous solution. be sure to add physical state symbols where appropriate.

Answer 1

Half reaction N_2 H_4  (aq)  →  N_2  (g)Balancing atoms except O and H N_2 H_4   (aq)  →   N_2  (g)Balancing charge N_2 H_4  (aq)→N_2  (g)+4H^+  (aq)Balanced half reaction for oxidation of hydrazine to gaseous nitrogen is N_2 H_4  (aq)→N_2  (g)+4 H^+  (aq)+  4e^-

Answer 2

Answer:Balanced half-reaction for the reduction of gaseous nitrogen to aqueous hydrazine is :

$N_2(g)+4H^+(aq)+4e^-\rightarrow N_2H_4(aq)$

Explanation:

Half reaction will be written as:

$N_2(g)\rightarrow N_2H_4(g)$

Balance the atoms in half reaction other than oxygen and hydrogen.

In acidic medium the hydrogen atom is balanced by adding $H^+$ ions.

$N_2(g)+4H^+(aq)\rightarrow N_2H_4(aq)$

Now balance the charge on both the sides by adding electrons on that side where positive charge is greater.

$N_2(g)+4H^+(aq)+4e^-\rightarrow N_2H_4(aq)$

Balanced half-reaction for the reduction of gaseous nitrogen to aqueous hydrazine is :

$N_2(g)+4H^+(aq)+4e^-\rightarrow N_2H_4(aq)$