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Chapter 3: Problem 13

The hemoglobin content of blood is about \(15.5 \mathrm{g} / 100 \mathrm{mL}\) blood. The molar mass of hemoglobin is about \(64,500 \mathrm{g} / \mathrm{mol},\) and there are four iron (Fe) atoms in a hemoglobin molecule. Approximately how many Fe atoms are present in the 6 Lof blood in a typical adult?

Short Answer

Expert verified
The number of Fe atoms present in the blood of a typical adult is approximately \(3.381 \times 10^{25}\)

Step by step solution

01

Convert the quantity of blood to mL

An adult has 6 L of blood, which converts to \(6000 \mathrm{mL}\) since \(1 \mathrm{L} = 1000 \mathrm{mL}\).
02

Find the mass of hemoglobin in this volume

If there is \(15.5 \mathrm{g}\) of hemoglobin in \(100 \mathrm{mL}\) of blood, then in \(6000 \mathrm{mL}\) of blood there will be \( \xi = \frac{6000 \times 15.5}{100} = 930 \mathrm{g} \) of hemoglobin, where \(\xi\) refers to the required quantity of hemoglobin.
03

Convert the mass of hemoglobin to moles

Knowing that the molar mass of hemoglobin is \(64500 \mathrm{g/mol}\), the molar quantity \(\eta\) of hemoglobin is found using the formula: \(\eta = \frac{\xi}{64500} = 0.014 \mathrm{mol}\)
04

Calculate the number of Fe atoms

Each molecule of hemoglobin contains 4 atoms of Fe. Therefore, the number of iron atoms is \(4 \times \eta \times 6.022 \times 10^{23} = 3.381 \times 10^{25}\)

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Most popular questions from this chapter

The compound \(\mathrm{C}_{7} \mathrm{H}_{7} \mathrm{NO}_{2}\) contains (a) 17 atoms per mole; (b) equal percents by mass of \(\mathrm{C}\) and \(\mathrm{H} ;\) (c) about twice the percent by mass of \(\mathrm{O}\) as of \(\mathrm{N} ;\) (d) about twice the percent by mass of \(\mathrm{N}\) as of \(\mathrm{H}\).

Name the acids: (a) \(\mathrm{HClO}_{2} ;\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{3} ;\) (c) \(\mathrm{H}_{2} \mathrm{Se}\) (d) HNO \(_{2}\).

The oxidation state of I in the ion \(\mathrm{H}_{4} \mathrm{IO}_{6}^{-}\) is (a) -1 (b) \(+1 ;(c)+7 ;(d)+8\)

A \(0.1888 \mathrm{g}\) sample of a hydrocarbon produces \(0.6260 \mathrm{g}\) \(\mathrm{CO}_{2}\) and \(0.1602 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\) in combustion analysis. Its molecular mass is found to be 106 u. For this hydrocarbon, determine its (a) mass percent composition; (b) empirical formula; (c) molecular formula.

An oxoacid with the formula \(\mathrm{H}_{x} \mathrm{E}_{y} \mathrm{O}_{z}\) has a formula mass of 178 u, has 13 atoms in its formula unit, contains \(34.80 \%\) by mass, and \(15.38 \%\) by number of atoms, of the element E. What is the element \(\mathrm{E}\), and what is the formula of this oxoacid?
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