Answer :
To determine which formula equation represents the burning of sulfur to produce sulfur dioxide, let's look closely at each chemical reaction option provided:
1. \( S (s) + O_2 (g) \xrightarrow{\Delta} SO_2 (g) \)
2. \( 2 H_2 S (s) + 3 O_2 (g) \longrightarrow 2 H_2 O (l) + 2 SO_2 (g) \)
3. \( 4 FeS_2 + 11 O_2 \longrightarrow 2 Fe_2 O_3 + 8 SO_2 \)
4. \( 2 SO_2 (g) + O_2 (g) \xrightarrow{V_2O_5} 2 SO_3 (g) \)
Let's analyze each option to identify the correct one:
1. The first reaction is:
\( S (s) + O_2 (g) \xrightarrow{\Delta} SO_2 (g) \)
This reaction shows sulfur (\(S\)) reacting directly with oxygen (\(O_2\)) to produce sulfur dioxide (\(SO_2\)). This perfectly matches the description.
2. The second reaction is:
\( 2 H_2 S (s) + 3 O_2 (g) \longrightarrow 2 H_2 O (l) + 2 SO_2 (g) \)
Here, hydrogen sulfide (\(H_2S\)) reacts with oxygen to produce water (\(H_2O\)) and sulfur dioxide (\(SO_2\)). While sulfur dioxide is produced, the reaction starts with hydrogen sulfide, not elemental sulfur.
3. The third reaction is:
\( 4 FeS_2 + 11 O_2 \longrightarrow 2 Fe_2 O_3 + 8 SO_2 \)
This reaction involves iron disulfide (\(FeS_2\)) reacting with oxygen to produce iron(III) oxide (\(Fe_2O_3\)) and sulfur dioxide (\(SO_2\)). Again, sulfur dioxide is produced, but the starting material is iron disulfide.
4. The fourth reaction is:
\( 2 SO_2 (g) + O_2 (g) \xrightarrow{V_2 O_5} 2 SO_3 (g) \)
This reaction shows sulfur dioxide reacting with oxygen in the presence of a vanadium(V) oxide catalyst to produce sulfur trioxide (\(SO_3\)). This does not describe the burning of elemental sulfur.
From the analysis, it is clear that the only equation that directly represents the burning of sulfur to produce sulfur dioxide is the first one:
[tex]\[ S (s) + O_2 (g) \xrightarrow{\Delta} SO_2 (g) \][/tex]
Thus, the formula that represents the burning of sulfur to produce sulfur dioxide is:
[tex]\[ S (s) + O_2 (g) \xrightarrow{\Delta} SO_2 (g) \][/tex]
1. \( S (s) + O_2 (g) \xrightarrow{\Delta} SO_2 (g) \)
2. \( 2 H_2 S (s) + 3 O_2 (g) \longrightarrow 2 H_2 O (l) + 2 SO_2 (g) \)
3. \( 4 FeS_2 + 11 O_2 \longrightarrow 2 Fe_2 O_3 + 8 SO_2 \)
4. \( 2 SO_2 (g) + O_2 (g) \xrightarrow{V_2O_5} 2 SO_3 (g) \)
Let's analyze each option to identify the correct one:
1. The first reaction is:
\( S (s) + O_2 (g) \xrightarrow{\Delta} SO_2 (g) \)
This reaction shows sulfur (\(S\)) reacting directly with oxygen (\(O_2\)) to produce sulfur dioxide (\(SO_2\)). This perfectly matches the description.
2. The second reaction is:
\( 2 H_2 S (s) + 3 O_2 (g) \longrightarrow 2 H_2 O (l) + 2 SO_2 (g) \)
Here, hydrogen sulfide (\(H_2S\)) reacts with oxygen to produce water (\(H_2O\)) and sulfur dioxide (\(SO_2\)). While sulfur dioxide is produced, the reaction starts with hydrogen sulfide, not elemental sulfur.
3. The third reaction is:
\( 4 FeS_2 + 11 O_2 \longrightarrow 2 Fe_2 O_3 + 8 SO_2 \)
This reaction involves iron disulfide (\(FeS_2\)) reacting with oxygen to produce iron(III) oxide (\(Fe_2O_3\)) and sulfur dioxide (\(SO_2\)). Again, sulfur dioxide is produced, but the starting material is iron disulfide.
4. The fourth reaction is:
\( 2 SO_2 (g) + O_2 (g) \xrightarrow{V_2 O_5} 2 SO_3 (g) \)
This reaction shows sulfur dioxide reacting with oxygen in the presence of a vanadium(V) oxide catalyst to produce sulfur trioxide (\(SO_3\)). This does not describe the burning of elemental sulfur.
From the analysis, it is clear that the only equation that directly represents the burning of sulfur to produce sulfur dioxide is the first one:
[tex]\[ S (s) + O_2 (g) \xrightarrow{\Delta} SO_2 (g) \][/tex]
Thus, the formula that represents the burning of sulfur to produce sulfur dioxide is:
[tex]\[ S (s) + O_2 (g) \xrightarrow{\Delta} SO_2 (g) \][/tex]
