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Which one of the following is least likely to be a product of a redox reaction between sulfuric acid and zinc metal? A - VCE - SSCE Chemistry - Question 9 - 2007 - Paper 1
Question 9
Which one of the following is least likely to be a product of a redox reaction between sulfuric acid and zinc metal? A. H₂ B. H₂S C. SO₂ D. SO₃
Worked Solution & Example Answer:Which one of the following is least likely to be a product of a redox reaction between sulfuric acid and zinc metal? A - VCE - SSCE Chemistry - Question 9 - 2007 - Paper 1
Step 1
Identify the Reaction Products
Answer
To analyze the redox reaction involving sulfuric acid (H₂SO₄) and zinc (Zn), we must recognize that zinc will reduce the sulfate ion (SO₄²⁻) to either sulfur dioxide (SO₂), hydrogen sulfide (H₂S), or potentially release hydrogen gas (H₂).
Zinc will oxidize to zinc ions (Zn²⁺) and we need to assess which product is least likely to occur from this process.
Step 2
Assess Each Product
Answer
- H₂: This can form from the reduction of protons in sulfuric acid, making it a feasible product.
- H₂S: This can occur if sulfate ions react under certain conditions, making this a possible product as well.
- SO₂: This can also form if sulfate is reduced during the reaction, thus making it a relevant product.
- SO₃: This is unlikely because sulfur(IV) would need to be oxidized to sulfur(VI), which does not typically occur in redox reactions between zinc and sulfuric acid.
Step 3