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Chapter 9: Problem 47

In words, what is the mass of 1 mole of atoms of any element?

Short Answer

Expert verified
The mass of 1 mole of atoms of any element is equal to its molar mass, which is the atomic weight of the element expressed in grams per mole (g/mol). For example, the mass of 1 mole of Carbon atoms is 12.01 g/mol.

Step by step solution

01

1. Identify the element and find their atomic weight

Choose any element from the periodic table, and look for its atomic weight (usually written below the symbol of the element). The atomic weight represents the average mass of one atom of the element in atomic mass units (amu). For example, let's use Carbon (C) as our chosen element. The atomic weight of Carbon is 12.01 amu.
02

2. Convert atomic weight to molar mass

Next, convert the atomic weight of the chosen element (which is in atomic mass units) to molar mass, which represents the mass of 1 mole of the element (in grams). 1 atomic mass unit (amu) is equal to 1 gram per mole (g/mol), so to convert amu to g/mol, we simply use the same numerical value but with different units. For Carbon, the molar mass is 12.01 g/mol.
03

3. Determine the mass of 1 mole of the chosen element

Now that we have the molar mass of the chosen element, we can say that the mass of 1 mole of atoms of that element is equal to the molar mass. For our example, the mass of 1 mole of Carbon atoms is 12.01 grams.

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Most popular questions from this chapter

Caffeine is made up of \(49.48 \%\) by mass \(C, 5.19 \%\) by mass \(\mathrm{H}, 28.85 \%\) by mass \(\mathrm{N}\), and \(16.48 \%\) by mass \(\mathrm{O}\). If its molar mass is approximately \(194 \mathrm{~g} / \mathrm{mol}\), what is the molecular formula of caffeine?

Determine the empirical formula of the compound that is \(43.2 \%\) by mass \(\mathrm{K}, 39.1 \%\) by \(\mathrm{mass} \mathrm{Cl}\), and also contains oxygen.

The compound naphthalene, which is used in mothballs, contains carbon, hydrogen, and possibly oxygen. When \(0.220 \mathrm{~g}\) of naphthalene is subjected to combustion analysis, it yields \(93.66 \% \mathrm{C}\) and \(6.31 \% \mathrm{H}\). If the molar mass of naphthalene is approximately \(128 \mathrm{~g} / \mathrm{mol}\), what is its molecular formula?

Chlorine \(\left(\mathrm{Cl}_{2}\right)\) and fluorine \(\left(\mathrm{F}_{2}\right)\) react to form \(\mathrm{ClF}_{3}\). A reaction vessel contains \(10.00 \mathrm{~g} \mathrm{Cl}_{2}\) and \(10.00 \mathrm{~g} \mathrm{~F}_{2}\). (Hint: Refer to Problem 9.82.) (a) Write a balanced chemical equation for this reaction. (b) Which reactant is limiting? (c) What is the theoretical yield for this reaction in grams? (d) How many grams of excess reactant are left over at the end of the reaction? (e) When this reaction is actually performed, \(12.50 \mathrm{~g}\) of \(\mathrm{ClF}_{3}\) is recovered. What is the percent yield of the reaction?

A \(2.000 \mathrm{~g}\) sample of a liquid compound that contains only carbon and hydrogen in its formula is subjected to combustion analysis. From the result, the lab determines that \(0.2874 \mathrm{~g}\) of the original sample's mass is due to hydrogen. (a) What is the percent by mass hydrogen for this sample? (b) What is the empirical formula for this compound? (c) The molar mass of this compound is determined to be about \(71 \mathrm{~g} / \mathrm{mol}\). What is the molecular formula for this compound?
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