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Chapter 10: Problem 83

What is the numerical value of Avogadro's number?

Short Answer

Expert verified
Avogadro's number is \( 6.022 \times 10^{23} \) particles/mol.

Step by step solution

01

Understanding Avogadro's Number

Avogadro's number is a fundamental constant in chemistry that represents the number of constituent particles, usually atoms or molecules, in one mole of a substance. It's named after the scientist Amedeo Avogadro.
02

Memorize Avogadro's Number

The exact value of Avogadro's number is a constant that students should memorize during their studies. It is an experimentally determined value.
03

Know the Exact Value

Avogadro's number is \[ 6.022 imes 10^{23} \] particles/mol. This means that one mole of any element or compound contains exactly \[ 6.022 imes 10^{23} \] of its atoms or molecules.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Mole Concept
The mole is a central concept in chemistry, designed to help chemists count tiny particles such as atoms and molecules in bulk amounts. Think of it as a bridge between the atomic world and the world we can measure and observe. A mole is like a chemist's dozen, but instead of 12, a mole represents about \( 6.022 \times 10^{23} \) particles. This number is essential in chemical equations and reactions, as it helps relate masses to number of particles.
  • The mole facilitates conversions between mass and number of particles.
  • One mole of any substance contains Avogadro's number of particles, be they atoms, molecules, ions, or other species.
  • The mole allows chemists to analyze reactions at the molecular level, even when dealing with macroscopic quantities.
Fundamental Constants
In the realm of chemistry and physics, fundamental constants such as Avogadro's number are values that remain the same across the universe. They are crucial because they provide a consistent foundation for scientific calculations and theories. Avogadro's number, \( 6.022 \times 10^{23} \) particles per mole, is particularly important in chemistry as it links the macroscopic world to the atomic scale.
Fundamental constants allow scientists to:
  • Consistently calculate the number of entities in large-scale chemical reactions.
  • Convert between atomic mass units and grams, facilitating the use of mass spectrometry and other analytical techniques.
  • Develop theoretical models that accurately predict substance behaviors at the molecular level.

Avogadro's constant is determined experimentally, often through methods involving crystal lattices and x-ray diffraction techniques, to provide precise values for scientific research.
Particles in a Mole
Avogadro's number, \( 6.022 \times 10^{23} \), specifies the quantity of particles contained within a mole. To grasp what this number means, consider:
  • It's the number of atoms in 12 grams of carbon-12, which serves as the neutral definition for the mole.
  • This vast number, though deceptively large, allows practical measurements of substances in labs and industry settings.
  • With each mole, you're counting a staggering amount of particles, enabling scientists to see the bigger picture in their experiments.

When working with this concept, envisioning everyday objects housing such vast counts of particles can be mind-boggling, yet it showcases chemistry's potential to manipulate and understand matter at the tiniest levels.

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Most popular questions from this chapter

Determine the percent composition of \(\mathrm{MgCO}_{3} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) and draw a pie graph to represent the hydrate.

Determine the number of oxygen atoms present in 25.0 g of carbon dioxide.

Express the composition of each compound as the mass percent of its elements (percent composition). \begin{equation} \begin{array}{l}{\text { a. sucrose }\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right) \quad \text { c. magnetite }\left(\mathrm{Fe}_{3} \mathrm{O}_{4}\right)} \\ {\text { b. aluminum sulfate }\left(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\right)}\end{array} \end{equation}

Which has more mass, a mole of potassium or a mole of sodium? Explain your answer.

Arrange these hydrates in order of increasing percent water content: \(\operatorname{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}, \mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O},\) and \(\mathrm{CoCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\)
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