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Chapter 3: Problem 9

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?

Short Answer

Expert verified
A mole is a unit in chemistry, defined as exactly 6.02214076 × 10^23 particles, with its unit usually represented as 'mol'. Similar to a pair, a dozen, and a gross, a mole signifies a quantity. Avogadro's number, which is equivalent to 6.02214076 × 10^23, signifies the number of particles in a mole.

Step by step solution

01

Defining Mole

The term 'mole' is a basic unit in chemistry. It is used to express amounts of a chemical substance and is defined as exactly 6.02214076 × 10^23 particles which could be atoms, molecules, ions, etc.
02

Identifying the Unit of Mole

The unit for mole in calculations is generally represented as 'mol'.
03

Connecting 'Mole' with Other Units

Similar to pair (2 units), dozen (12 units), and gross (144 units), a mole is just another way to express a quantity - in this case, it's a very large quantity: 6.02214076 × 10^23 units. These terms provide a quantity of items (two in a pair, twelve in a dozen, etc.), and a mole represents Avogadro's number of particles.
04

Understanding Avogadro's Number

Avogadro's number, also known as Avogadro's constant, represents the number of particles in one mole of a substance. It is numerically equal to 6.02214076 × 10^23 and was named after scientist Amedeo Avogadro.

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Most popular questions from this chapter

(a) For molecules having small molecular masses, mass spectrometry can be used to identify their formulas. To illustrate this point, identify the molecule that most likely accounts for the observation of a peak in a mass spectrum at 16 amu, 17 amu, 18 amu, and 64 amu. (b) Note that there are (among others) two likely molecules that would give rise to a peak at 44 amu, namely, \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(\mathrm{CO}_{2} .\) In such cases, a chemist might try to look for other peaks generated when some of the molecules break apart in the spectrometer. For example, if a chemist sees a peak at 44 amu and also one at 15 amu, which molecule is producing the 44 -amu peak? Why? (c) Using the following precise atomic masses \(-\mathrm{H}\) ( 1.00797 amu), \({ }^{12} \mathrm{C}(12.00000 \mathrm{amu}),\) and \({ }^{16} \mathrm{O}(15.99491 \mathrm{amu})-\) how precisely must the masses of \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(\mathrm{CO}_{2}\), be measured to distinguish between them?

Describe the steps involved in the mole method.

The empirical formula of a compound is CH. If the molar mass of this compound is about \(78 \mathrm{~g},\) what is its molecular formula?

Consider the combustion of carbon monoxide (CO) in oxygen gas: $$2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)$$Starting with 3.60 moles of \(\mathrm{CO}\), calculate the number of moles of \(\mathrm{CO}_{2}\) produced if there is enough oxygen gas to react with all of the CO.

A sample containing \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{SO}_{4},\) and \(\mathrm{NaNO}_{3}\) gives the following elemental analysis: Na: 32.08 percent; O: 36.01 percent; Cl: 19.51 percent. Calculate the mass percent of each compound in the sample.
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