A mixture of FeO and `Fe_(2)O_(3)` is reacted with acidified `KMnO_(4)` solution having a concentration of 0.2278 M, 100 ml of which was used. The solution was then titrated with Zn dust which converted `Fe_(2+)` of the solution to `Fe^(2+)`. The `Fe^ (2+)` required 1000 ml of 0.13 M `K_(2)Cr_(2) O_(7)` solution. Find the % of FeO & `Fe_(2)O_(3)`.

Explanation

To solve the problem step by step, we will follow the outlined process in the video transcript.

### Step 1: Calculate the milliequivalents of KMnO4 used
Given:
- Molarity of KMnO4 = 0.2278 M
- Volume of KMnO4 = 100 mL = 0.1 L

The number of equivalents of KMnO4 can be calculated using the formula:
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