Question

Calculate the oxidation number of sulfur in \( \text{H}_2\text{SO}_4 \).

• A. +4
• B. +6
• C. +2
• D. 0

Hint:

Remember: The oxidation number of oxygen is typically \( -2 \), and hydrogen is \( +1 \). Use the sum of oxidation states in a neutral compound to solve for unknown oxidation numbers.

Answer 1

The Correct Option is B

Step 1: Assign oxidation numbers to known elements In \( \text{H}_2\text{SO}_4 \), hydrogen (\( H \)) has an oxidation state of \( +1 \) and oxygen (\( O \)) has an oxidation state of \( -2 \).Step 2: Set up the equation for the sum of oxidation states Assign \( x \) as the oxidation state of sulfur. For a neutral compound like \( \text{H}_2\text{SO}_4 \), the sum of oxidation states is zero.\[2(\text{oxidation state of H}) + (\text{oxidation state of S}) + 4(\text{oxidation state of O}) = 0\]Substitute known values:\[2(1) + x + 4(-2) = 0\]\[2 + x - 8 = 0\]\[x - 6 = 0\]\[x = +6\]Answer: The oxidation number of sulfur in \( \text{H}_2\text{SO}_4 \) is +6. The correct answer is option (2).