Question

Find the values of a, b, c, and d for the following redox equation: $ a\text{I}_2 + b\text{NO} + 4\text{H}_2\text{O} = c\text{HNO}_3 + d\text{HI} $

• A. 3, 2, 2, 6
• B. 2, 3, 2, 6
• C. 3, 2, 6, 2
• D. 6, 3, 2, 2

Hint:

Balancing redox reactions requires balancing both mass and charge. Split the reaction into oxidation and reduction half-reactions, and then balance them.

Answer 1

The Correct Option is A

To balance this redox reaction, first break it down into the half-reactions. The oxidation half-reaction involves \( \text{I}_2 \) being reduced to \( \text{HI} \), and the reduction half-reaction involves \( \text{NO} \) being oxidized to \( \text{HNO}_3 \). Oxidation half-reaction: \[ \text{I}_2 + 2\text{e}^- \rightarrow 2\text{I}^- \] Reduction half-reaction: \[ \text{NO} + 2\text{H}_2\text{O} \rightarrow \text{HNO}_3 + 2\text{e}^- \] After balancing the atoms and charges, we find the coefficients: \( a = 3 \), \( b = 2 \), \( c = 2 \), and \( d = 6 \).