Answer:
NO2(g) + H2O(l) → NO3-(aq) + 2 H+(aq) + 1 e-
Explanation:
Let’s balance the half reaction step by step (in an acidic solution):
• Balance the non-hydrogen and non-oxygen elements first
NO2(g) → NO3-(aq) (N: balanced)
• Balance oxygen by adding H2O to the side that needs oxygen (1 O : 1 H2O)
NO2(g) + H2O(l) → NO3-(aq)
• Balance hydrogen by adding H+ to the side that needs hydrogen (1 H : 1 H+)
NO2(g) + H2O(l) → NO3-(aq) + 2 H+(aq)
• Balance the charges: add electrons to the more positive side (or less negative side)
NO2(g) + H2O(l) → NO3-(aq) + 2 H+(aq)
Reactants Products
0 (-1) + (+1 x 2) = +1
+ 1 e- ____ _______
0
NO2(g) + H2O(l) → NO3-(aq) + 2 H+(aq) + 1 e- → balanced half reaction
The problem mentioned that the half reaction is an oxidation reaction, and the balanced reaction is an oxidation reaction because it lost an electron
The required balanced half- reaction equation is NO2(g) + H2O(l) ------> NO3^-(aq) + 2H^+(aq) + e
A redox reaction is one in which there is loss and gain of electrons. One specie looses electrons and another specie gains electrons. The change from nitrogen dioxide to nitrate ion is an oxidation reaction. The oxidation number of nitrogen increases from +4 to +5 hence one electron was lost.
The balanced half-reaction for the oxidation of gaseous nitrogen dioxide to nitrate ion in acidic aqueous solution is;
NO2(g) + H2O(l) ------> NO3^-(aq) + 2H^+(aq) + e
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