Balance the redox reaction with oxidation number method:(with full method)
FeCl3+H2S=FeCl2+HCL+S
Answers
Answer:
FeCl₃ + H₂S → FeCl₂ + HCl + S
Step 1: Assign oxidation numbers to each of the atoms in the equation and write the numbers above the atom.
Fe₂⁺³Cl₃⁻¹ + H₂⁺¹S⁻¹ → Fe⁻²Cl₂⁻¹ + H⁺¹Cl⁻¹ + S⁰
Step 2: Identify the atoms that are oxidized and those that are reduced. In the above equation, the sulphur atom is being oxidized since its oxidation number increases from -2 to 0. The iron atom is being reduced since its oxidation number decreases from +3 to +2.
O: H₂⁺¹S⁻² → S⁰ + 2e⁻
R: Fe⁺³Cl₃⁻¹ + e⁻ → Fe⁺²Cl₂⁻¹
Step 3. Balance the atoms in each half reaction.
O: H₂⁺¹S⁻² → S⁰ + 2e⁻ + 2H⁺
R: Fe⁺³Cl₃⁻¹ + e⁻ + H⁺ → Fe⁺²Cl₂⁻¹ + HCl
Step 4. Make electron gain equivalent to electron lost.
now, our goal is to eliminate e⁻ and H⁺
⇒
(O: H₂⁺¹S⁻² → S⁰ + 2e⁻ + 2H⁺) × 1
(R: Fe⁺³Cl₃⁻¹ + e⁻ + H⁺ → Fe⁺²Cl₂⁻¹ + HCl) × 2
⇒
O: H₂⁺¹S⁻² → S⁰ + 2e⁻ + 2H⁺
R: 2 Fe⁺³Cl₃⁻¹ + 2e⁻ + 2H⁺ → 2 Fe⁺²Cl₂⁻¹ + 2HCl
Step 5. Add the half-reactions together.
⇒
H₂⁺¹S⁻² + 2 Fe⁺³Cl₃⁻¹ + 2e⁻ + 2H⁺ → S⁰ + 2e⁻ + 2H⁺ + 2 Fe⁺²Cl₂⁻¹ + 2HCl
Step 6. Simplify the equation.
⇒ H₂⁺¹S⁻² + 2 Fe⁺³Cl₃⁻¹ → S⁰ + 2 Fe⁺²Cl₂⁻¹ + 2HCl
Step 7. Write the simplified equation obtained without oxidation numbers.
⇒ H₂S + 2FeCl₃ → S + 2FeCl₂ + 2HCl
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