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Chapter 9: Problem 42

How many \(\mathrm{O}_{2}\) molecules are there in 1 mole of \(\mathrm{O}_{2}\) molecules? How many \(\mathrm{O}\) atoms are there in 1 mole of \(\mathrm{O}_{2}\) molecules?

Short Answer

Expert verified
In 1 mole of O₂ molecules, there are \(6.022 \times 10^{23}\) O₂ molecules and \(1.2044 \times 10^{24}\) O atoms.

Step by step solution

01

Recall the definition of a mole and Avogadro's number

A mole is the amount of substance that contains as many particles (such as atoms, molecules, ions, etc.) as there are in 12 grams of pure carbon-12. Avogadro's number (Nₐ) is the number of particles in one mole of a substance and is equal to 6.022 x 10²³ particles per mole.
02

Find the number of O₂ molecules in 1 mole of O₂ molecules

Since there are 6.022 x 10²³ particles in 1 mole of a substance, there are 6.022 x 10²³ O₂ molecules in 1 mole of O₂ molecules.
03

Find the number of O atoms in 1 mole of O₂ molecules

In one O₂ molecule, there are 2 O atoms. Since there are 6.022 x 10²³ O₂ molecules in 1 mole of O₂ molecules, we can multiply this number by the number of O atoms in each O₂ molecule to find the number of O atoms in 1 mole of O₂ molecules: \( (6.022 \times 10^{23}) \times 2 = 1.2044 \times 10^{24} \) O atoms. In conclusion, there are 6.022 x 10²³ O₂ molecules in 1 mole of O₂ molecules, and there are 1.2044 x 10²⁴ O atoms in 1 mole of O₂ molecules.

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Most popular questions from this chapter

Consider the following unbalanced chemical equation: \(\mathrm{H}_{2}+\mathrm{N}_{2} \rightarrow \mathrm{NH}_{3}\) (a) To run this reaction in a balanced fashion, how much nitrogen is required if you start with \(10.0 \mathrm{~g}\) of \(\mathrm{H}_{2} ?\) (b) How many grams of ammonia \(\left(\mathrm{NH}_{3}\right)\) will you produce if you run the reaction with the masses calculated in part (a)? (c) How many molecules of ammonia will you produce?

Ethylene glycol, used for antifreeze, has the molecular formula \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\). Calculate the mass percent of each element in ethylene glycol.

Vitamin \(\mathrm{C}\), also known as ascorbic acid, contains carbon, hydrogen, and possibly oxygen. A \(0.160 \mathrm{~g}\) sample of ascorbic acid is subjected to combustion analysis, yielding \(40.93 \%\) C and \(4.58 \%\) H. If the molar mass of ascorbic acid is approximately \(176 \mathrm{~g} / \mathrm{mol}\), what is its molecular formula?

If you have \(44.6 \mathrm{~g}\) of carbon tetrachloride, how many atoms of chlorine do you have?

A \(1.540-g\) sample of a liquid is subjected to combustion analysis, yielding \(40.00 \% \mathrm{C}\) and \(6.71 \% \mathrm{H}\). It may also contain oxygen. (a) What is the empirical formula for this compound? (b) The molar mass of this compound is determined to be about \(30 \mathrm{~g} / \mathrm{mol}\). What is the molecular formula for this compound?
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