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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

An impure sample of zinc \((\mathrm{Zn})\) is treated with an excess of sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) to form zinc sulfate \(\left(\mathrm{ZnSO}_{4}\right)\) and molecular hydrogen \(\left(\mathrm{H}_{2}\right) .\) (a) Write a balanced equation for the reaction. (b) If \(0.0764 \mathrm{~g}\) of \(\mathrm{H}_{2}\) is obtained from \(3.86 \mathrm{~g}\) of the sample, calculate the percent purity of the sample. (c) What assumptions must you make in (b)?

Urea \(\left[\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}\right]\) is used for fertilizer and many other things. Calculate the number of \(\mathrm{N}, \mathrm{C}, \mathrm{O},\) and \(\mathrm{H}\) atoms in \(1.68 \times 10^{4} \mathrm{~g}\) of urea.

How many atoms are there in 5.10 moles of sulfur (S)?

The atomic masses of \({ }_{17}^{35} \mathrm{Cl}(75.53\) percent \()\) and \({ }_{17}^{37} \mathrm{Cl}\) (24.47 percent) are 34.968 amu and 36.956 amu, respectively. Calculate the average atomic mass of chlorine. The percentages in parentheses denote the relative abundances.

Why is the theoretical yield of a reaction determined only by the amount of the limiting reagent?
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