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Determine the empirical formula of an oxide of iron which has iron and dioxygen by mass.
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The iron oxide has 69.9% iron and 30.1% dioxygen by mass.
Thus, 100 g of iron oxide contains 69.9 g iron and 30.1 g dioxygen.
The number of moles of iron present in 100 g of iron oxide are .
The number of moles of dioxygen present in 100 g of iron oxide are .
The ratio of the number of oxygen atoms to the number of iron atoms present in one formula unit of iron oxide is .
Hence, the formula of the iron oxide is .
Thus, 100 g of iron oxide contains 69.9 g iron and 30.1 g dioxygen.
The number of moles of iron present in 100 g of iron oxide are .
The number of moles of dioxygen present in 100 g of iron oxide are .
The ratio of the number of oxygen atoms to the number of iron atoms present in one formula unit of iron oxide is .
Hence, the formula of the iron oxide is .
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Question Text | Determine the empirical formula of an oxide of iron which has iron and dioxygen by mass. |
Updated On | Oct 23, 2023 |
Topic | Some Basic Concepts of Chemistry |
Subject | Chemistry |
Class | Class 11 |
Answer Type | Text solution:1 Video solution: 48 |
Upvotes | 4830 |
Avg. Video Duration | 5 min |