Step 1: Determine the atomic composition of \( \text{H}_2\text{SO}_4 \).\( \text{H}_2\text{SO}_4 \) contains:- 2 hydrogen atoms (\( \text{H} \)),- 1 sulfur atom (\( \text{S} \)),- 4 oxygen atoms (\( \text{O} \)).Step 2: Establish known oxidation states.The oxidation state of hydrogen (\( \text{H} \)) is \( +1 \).The oxidation state of oxygen (\( \text{O} \)) is \( -2 \).Step 3: Formulate the equation to solve for sulfur's oxidation state.The sum of oxidation states in a neutral molecule is 0. Let \( x \) represent the oxidation state of sulfur.For \( \text{H}_2\text{SO}_4 \), the equation is:\[2(+1) + x + 4(-2) = 0\]Solving the equation:\[2 + x - 8 = 0\]\[x = 6\] Answer: The oxidation state of sulfur in \( \text{H}_2\text{SO}_4 \) is \( +6 \).