H₂O₂ + ClO₂ → ClO₂^– + O₂ + H₂O
What is the equivalent weight of reductant?

Options:

1. 17

2. 34

3. 67.5

4. 33.75

To determine the equivalent weight of the reductant in the reaction you provided, we first need to analyze the chemical equation: H2O2 + ClO2 → ClO2– + O2 + H2O. In this reaction, hydrogen peroxide (H2O2) acts as a reductant, meaning it donates electrons and gets oxidized. Let's break down the steps to find the equivalent weight.

Understanding Equivalent Weight

The equivalent weight of a substance is calculated using the formula:

Equivalent Weight = Molar Mass / n

Here, n represents the number of electrons transferred per mole of the substance in the reaction.

Step 1: Determine the Molar Mass of H2O2

The molar mass of hydrogen peroxide (H2O2) can be calculated as follows:

• Hydrogen (H): 1 g/mol × 2 = 2 g/mol
• Oxygen (O): 16 g/mol × 2 = 32 g/mol

Adding these together gives:

Molar Mass of H2O2 = 2 + 32 = 34 g/mol

Step 2: Identify the Change in Oxidation State

In this reaction, hydrogen peroxide is oxidized to oxygen (O2). The oxidation state of oxygen in H2O2 is -1, and in O2, it is 0. Therefore, each molecule of H2O2 loses 2 electrons (since there are two oxygen atoms). Thus, n = 2.

Step 3: Calculate the Equivalent Weight

Now that we have the molar mass and the number of electrons transferred, we can calculate the equivalent weight:

Equivalent Weight = Molar Mass / n = 34 g/mol / 2 = 17 g/equiv

Final Answer

The equivalent weight of the reductant (H2O2) in this reaction is 17. Therefore, the correct option is 1. 17.

This calculation illustrates how understanding the oxidation states and the concept of equivalent weight can help in analyzing redox reactions effectively. If you have any further questions about this topic or related concepts, feel free to ask!