Step 1: Assign oxidation numbers to the elements in \( \text{H}_2\text{SO}_4 \) The oxidation number for hydrogen \( \text{H} \) is \( +1 \), and for oxygen \( \text{O} \) is \( -2 \). Step 2: Apply the rule for the sum of oxidation numbers The sum of oxidation numbers in a neutral compound equals zero. The two hydrogen atoms contribute \( +2 \). The four oxygen atoms contribute \( 4 \times (-2) = -8 \). Let \( x \) represent the oxidation number of sulfur.\[2 \times (+1) + x + 4 \times (-2) = 0\]\[2 + x - 8 = 0\]\[x = +6\]Answer: The oxidation number of sulfur in \( \text{H}_2\text{SO}_4 \) is \( +6 \). This corresponds to option (1).