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Chapter 1: Problem 86

Measurements show that \(1.0 \mathrm{~g}\) of iron (Fe) contains \(1.1 \times 10^{22}\) Fe atoms. How many Fe atoms are in \(4.9 \mathrm{~g}\) of Fe, which is the total amount of iron in the body of an average adult?

Short Answer

Expert verified
To find the total number of atoms in \(4.9 \mathrm{~g}\) of iron, multiply \(4.9\) by the conversion factor. The number of iron atoms in an average adult body is \(5.39 \times 10^{22}\).

Step by step solution

01

Determine Conversion Factor

The exercise tells you that one gram of iron contains \(1.1 \times 10^{22}\) Fe atoms. This is the conversion factor.
02

Set up Proportion

If 1.0 g of iron contains \(1.1 \times 10^{22}\) iron atoms, then \(4.9 \mathrm{~g}\) of iron contains an unknown number of iron atoms (let's denote this quantity by \(X\)). You can set up a proportion:\[ \frac{4.9}{1} = \frac{X}{1.1 \times 10^{22}}\]
03

Solve for X

To solve for \(X\), cross-multiply and divide:\[X = 4.9 \times (1.1 \times 10^{22})\]

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Most popular questions from this chapter

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