   Chapter 2, Problem 126GQ

Chapter
Section
Textbook Problem

Your doctor has diagnosed you as being anemic–that is, as having too little iron in your blood. At the drugstore, you find two iron-containing dietary supplements: one with iron(II) sulfate, FeSO4, and the other with iron(II) gluconate. Fe(C6H11 O7)2. 1fyou take 100. mg of each compound, which will deliver more atoms of iron?

Interpretation Introduction

Interpretation: It should be determined that which of the given compound will deliver more atoms of iron.

Concept introduction:

• Moleofsubstance=GramofsubstanceMolarmass
• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol)
• Mass percentage is one way to represent the concentration of an element in a compound or a component in a mixture. Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.
Explanation

Two iron containing dietary supplements are given,

One with iron (II) sulfate FeSO4 and the other with iron (II) gluconate Fe(C6H11O7)2

The molar mass of FeSO4 is 151.908g/mol

The molar mass of Fe(C6H11O7)2 is 448.156g/mol

The mass percent of iron element in these compounds can be determined as follows,

MolarMassofIroninFeSO4 =1×55.845=55.845g/molMasspercentofIroninFeSO4=MolarmassofIronMolarmassofFeSO4×100 =55.845151.908×100 =36.76%

Mass of iron in FeSO4 is,

36.76100×100mg=36.76mg

The number of atoms of iron delivered from FeSO4 is,

0.03676g55.845g/molFe×6.022×1023=3.96×1020atomFe

Similarly,

MolarMassofIroninFe(C6H11O7)2 =1×55

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