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 \( \text{H}_2\text{SO}_4 \), the oxidation state of hydrogen (\( H \)) is \( +1 \) and the oxidation state of oxygen (\( O \)) is \( -2 \). Step 2: Set up the equation for the sum of oxidation states Let the oxidation state of sulfur be \( x \). The sum of the oxidation states in \( \text{H}_2\text{SO}_4 \) must equal zero because it is a neutral compound. \[ 2(\text{oxidation state of H}) + (\text{oxidation state of S}) + 4(\text{oxidation state of O}) = 0 \] Substitute the known oxidation states: \[ 2(1) + x + 4(-2) = 0 \] \[ 2 + x - 8 = 0 \] \[ x - 6 = 0 \] \[ x = +6 \] Answer: Therefore, the oxidation number of sulfur in \( \text{H}_2\text{SO}_4 \) is +6. So, the correct answer is option (2).