Question

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.

Answer 1

Answer:

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-

Answer 2

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-

• The first step involves reaction of arsine with water

AsH₃(g) + 4H₂O(l) -----> H₃AsO₄(aq)

• The second step involves balancing oxygen using hydrogen ions

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

• The third and final step involves noting the the number of electrons transferred in the redox reaction

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

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