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Chapter 4

Q. 4.7

Consider the unbalanced redox equation:

Cr^{3+}(aq) + H_{2}O_{2}(aq) → 2H_{2}O + Cr_{2}O_{7}^{2-}(aq)

(a) Identify the element oxidized and the element reduced.

(b) What are the oxidizing and reducing agents?

STRATEGY

1. Determine the oxidation number of each element.
2. Find elements whose oxidation numbers change.

Step-by-Step

Verified Solution

Cr: +3; H: +1; O: -1 → H: +1; O: -2; Cr: +6 Oxidation numbers
Cr: +3 → +6 (increase)

O: -1 → -2 (decrease)

Change
O (decrease in oxidation number) Element reduced
Cr (increase in oxidation number) Element oxidized
H_{2}O_{2} (It is the species that contains the element that is reduced.) Oxidizing agent
Cr_{2}O_{7}^{2-} (It is the species that contains the element that is oxidized.) Reducing agent