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Chapter 3: Problem 4

What information would you need to calculate the average atomic mass of an element?

Short Answer

Expert verified
To calculate the average atomic mass of an element, one needs to know the atomic mass of each isotope of the element and the relative abundance of each isotope.

Step by step solution

01

Understand the constituents of average atomic mass

In order to calculate the average atomic mass of an element, one must be familiar with the concept of isotopes, which are varieties of an element that differ in neutron number, and thus mass number, but not in proton number. An element's isotopes each contribute to its average atomic mass.
02

Identify the necessary information

The information required to calculate the average atomic mass of an element includes the exact atomic mass of each isotope (in atomic mass units), as well as the relative abundance of each isotope expressed either as a percentage or a decimal fraction.
03

Understand the calculation process

The calculation of the average atomic mass involves multiplying each isotope's atomic mass by its relative abundance, then summing these results. Here, the relative abundance acts like a weighting factor to reflect the proportion of that isotope present in a given sample of the element.

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Most popular questions from this chapter

The atomic masses of \({ }_{3}^{6} \mathrm{Li}\) and \({ }_{3}^{7} \mathrm{Li}\) are \(6.0151 \mathrm{amu}\) and 7.0160 amu, respectively. Calculate the natural abundances of these two isotopes. The average atomic mass of Li is 6.941 amu.

Which of the following has a greater mass: 2 atoms of lead or \(5.1 \times 10^{-23}\) mole of helium?

Consider the combustion of butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right)\) : $$ 2 \mathrm{C}_{4} \mathrm{H}_{10}(g)+13 \mathrm{O}_{2}(g) \longrightarrow 8 \mathrm{CO}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(l) $$ In a particular reaction, 5.0 moles of \(\mathrm{C}_{4} \mathrm{H}_{10}\) are reacted with an excess of \(\mathrm{O}_{2}\). Calculate the number of moles of \(\mathrm{CO}_{2}\) formed.

Describe how the knowledge of the percent composition by mass of an unknown compound can help us identify the compound.

Define the term "mole." What is the unit for mole in calculations? What does the mole have in common with the pair, the dozen, and the gross? What does Avogadro's number represent?
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