
Concept explainers
Interpretation:
The molar mass, percent composition, and empirical formula of ferrous fumarate and the mass of
Concept Introduction:
The molar mass is calculated by adding the masses of each and every element multiplied by their number of atoms present (given in subscript). Its S.I. unit is
To calculate the empirical formula, the use of combustion analysis is done. In this method, the number of moles of each element is calculated by using the given information, and then it is divided by the least number of moles of element present in the reaction. After that, it is converted into the smallest whole number ratio.
The molecular formula is a whole number, multiple of empirical formula, given by the expression, which is as follows:
The percent composition of an element by its mass in a compound is calculated by the formula, given as follows:
where, n represents the elements and the number of atoms in the given molecule or compound.

Answer to Problem 160AP
Solution:
a)
Molar mass
b)
c)
The mass of
d)
The mass of iron present in the tablet is
Explanation of Solution
a) The molar mass and percent composition of ferrous fumarate
The molar mass is calculated by adding the masses of each and every element multiplied by their number of atoms present (given in subscript). Its S.I. unit is
So, the molar mass of ferrous fumarate is calculated as follows:
The percent composition of an element in a compound is given by the expression, which is as follows:
The mass percent of
The mass percent of
The mass percent of
The mass percent of
b) Empirical formula of ferrous fumarate
The molecular formula is given by the expression, as follows:
As, the molecular formula of ferrous fumarate is
The whole number,
The greatest common factor of
The empirical formula of the compound is given as follows:
c) Mass of
The balanced equation for the combustion of
Since the molar ratio of
So, the number of moles of
The number of moles of
Substitute
Therefore, the number of moles of
The mass of
Substitute
Similarly, the molar ratio of
So, the number of moles of
The number of moles of
Substitute
Therefore, the number of moles of
The mass of
Substitute
Hence, the mass of
d)It is not necessary for the tablets in the photograph to be in unit-dose blister packaging.
The mass of tablet is
Iron in unit-blister packaging is more than
The percentage of Fe in
So, the mass of iron present in the tablet is calculated as follows:
It is clearly seen that this mass is less than 30 mg. Hence, it is not important to pack them in the unit–blister.
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Chapter 3 Solutions
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