Given below are two statements:
Statement I: In the metallurgy process, sulphide ore is converted to oxide before reduction.
Statement II: Oxide ores in general are easier to reduce.
In the light of the above statements, choose the most appropriate answer from the options below:

We need to evaluate two statements about metallurgy.

Statement I: In the metallurgy process, sulphide ore is converted to oxide before reduction.

This is correct. The process of converting sulphide ores to oxides is called roasting. For example:

$$ 2ZnS + 3O_2 \xrightarrow{\Delta} 2ZnO + 2SO_2 $$

$$ 2PbS + 3O_2 \xrightarrow{\Delta} 2PbO + 2SO_2 $$

After roasting, the metal oxide is then reduced to the metal using a suitable reducing agent (carbon, CO, or another metal).

Statement II: Oxide ores in general are easier to reduce.

This is correct. Metal oxides are thermodynamically easier to reduce than metal sulphides for several reasons:

1. Carbon and CO are readily available, cheap reducing agents that can reduce most metal oxides at reasonable temperatures.

2. On the Ellingham diagram, the line for $$2C + O_2 \to 2CO$$ has a negative slope, meaning carbon becomes a better reducing agent at higher temperatures, and it falls below most metal oxide lines.

3. Direct reduction of sulphides is difficult because the corresponding reactions are less thermodynamically favourable.

Both statements are correct, and Statement II provides the reason for the practice described in Statement I.

The correct answer is Option 4: Both Statement I and Statement II are correct.