Question

In the given Redox equation, identify the stoichiometric coefficients w, x, y, and z.
The given equation: \[ \text{ClO}_3^{-} + w\text{Cl}^{-} + x\text{H}^{+} \rightarrow y\text{H}_2\text{O} + z\text{Cl}_2 \]

• A. \( w = 3 \), \( x = 6 \), \( y = 3 \), \( z = 2 \)
• B. \( w = 5 \), \( x = 6 \), \( y = 3 \), \( z = 3 \)
• C. \( w = 6 \), \( x = 6 \), \( y = 3 \), \( z = 4 \)
• D. \( w = 6 \), \( x = 5 \), \( y = 2.5 \), \( z = 3 \)

Hint:

When balancing redox reactions, always check both mass and charge balance for each element and ion.

Answer 1

The Correct Option is B

To solve this, we need to balance both mass and charge in the redox equation. Here's the step-by-step process: - Step 1: Analyze oxidation states and half-reactions The chlorine in \( \text{ClO}_3^{-} \) has an oxidation state of +5, while in \( \text{Cl}_2 \), it has an oxidation state of 0. This indicates that chlorine is reduced in the reaction. - Step 2: Balance chlorine atoms We have one chlorine atom in \( \text{ClO}_3^{-} \) on the left and two chlorine atoms in \( \text{Cl}_2 \) on the right. Therefore, the coefficient \( z \) must be 3 to balance the chlorine atoms. - Step 3: Balance hydrogen atoms There are \( y \) molecules of \( \text{H}_2\text{O} \) on the right, and each molecule contains two hydrogen atoms. To balance the hydrogen atoms on both sides, set \( y = 3 \). - Step 4: Balance charges The charges on the left side are as follows: - \( \text{ClO}_3^{-} \) has a charge of -1, - \( w \) \( \text{Cl}^{-} \) ions contribute a charge of -1 each, - \( x \) \( \text{H}^{+} \) ions contribute a charge of +1 each. On the right side, the products are neutral (\( \text{H}_2\text{O} \) and \( \text{Cl}_2 \) are neutral). To balance the charges, set \( w = 5 \) and \( x = 6 \). This ensures that the charges on both sides of the equation are equal. Thus, the stoichiometric coefficients are \( w = 5 \), \( x = 6 \), \( y = 3 \), and \( z = 3 \).