Write a balanced half-reaction for the oxidation of gaseous arsine AsH3 to aqueous arsenic acid H3AsO4 in acidic aqueous solution. Be sure to add physical state symbols where appropriate.

The balanced half-reaction for the oxidation of gaseous arsine AsH₃ to

aqueous arsenic acid H₃AsO₄ in acidic aqueous solution is

AsH₃(g) + 4H₂O(l)> H₃AsO₄(aq) +8H+(aq) + 8e-

AsH₃(g) + 4H₂O(l) > H₃AsO₄(aq)

AsH₃(g) + 4H₂O(l)> H₃AsO₄(aq) +8H⁺(aq)

AsH₃(g) + 4H₂O(l)> H₃AsO4(aq) +8H⁺(aq) + 8e⁻

Read more on link

AsH3(g) + 4H2O(l)> H3AsO4(aq) +8H^+(aq) + 8e-

Explanation:

Now we need to work through the problem in steps.

Step1: reaction of arsine with water

AsH3(g) + 4H2O(l) > H3AsO4(aq) this is the molecular reaction

Step II: oxygen is balanced using hydrogen ions

AsH3(g) + 4H2O(l)> H3AsO4(aq) +8H^+(aq)

Step III: We specify the number of electrons transferred in the redox reaction

AsH3(g) + 4H2O(l)> H3AsO4(aq) +8H^+(aq) + 8e-

c. orbital shape i hope this is correct