Question

which formula equation represents the burning of sulfur to produce sulfur dioxide?
\\(\ce{s(s) + o_{2}(g) ->\delta so_{2}(g)}\\)
\\(\ce{2h_{2}s(s) + 3o_{2}(g) -> 2h_{2}o(l) + 2so_{2}(g)}\\)
\\(\ce{4fes_{2} + 11o_{2} -> 2fe_{2}o_{3} + 8so_{2}}\\)
\\(\ce{2so_{2}(g) + o_{2}(g) ->v_{2}o_{5} 2so_{3}(g)}\\)

Explanation:

To determine the correct formula equation for the burning of sulfur to produce sulfur dioxide, we analyze each option:

• The first option: \( \text{S(s)} + \text{O}_2\text{(g)} \xrightarrow{\Delta} \text{SO}_2\text{(g)} \) shows solid sulfur (\( \text{S} \)) reacting with gaseous oxygen (\( \text{O}_2 \)) (burning) to form gaseous sulfur dioxide (\( \text{SO}_2 \)), which matches the description.
• The second option involves \( \text{H}_2\text{S} \) (hydrogen sulfide), not pure sulfur, so it is incorrect.
• The third option involves \( \text{FeS}_2 \) (iron disulfide), not pure sulfur, so it is incorrect.
• The fourth option shows the reaction of \( \text{SO}_2 \) with \( \text{O}_2 \) to form \( \text{SO}_3 \), which is not the burning of sulfur to form \( \text{SO}_2 \).

Answer:

A. \( \text{S(s)} + \text{O}_2\text{(g)} \xrightarrow{\Delta} \text{SO}_2\text{(g)} \)