Name: mole, mass, and avogadro’s number
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 1 min 54 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.2.1

Molar Mass

Periyodik tablo, her atomun ortalama atom kütlesini verir. Bununla birlikte, makroskopik örnekler çok fazla sayıda atom içerir. Bu nedenle, Avogadro sayısı adı verilen bir sayma birimi kullanmak mantıklıdır.NA sembolü olarak ifade edilen Avogadro sayısı genellikle 6, 022 X 10^23'e yuvarlanır. Değeri, tam olarak 12 gram saf karbon-12 izotopundaki atom sayısına eşittir. Mol terimi, Avogadro sayısını tanımlamak için kullanılır, tıpkı bilindik bir terim olan düzinenin, 12 sayısını tanımlamak için kullanıldığı gibi.Bununla birlikte, bir düzine farklı madde, aynı sayıda maddeye sahip olmasına rağmen farklı ağırlıkta olabilir. Benzer şekilde, farklı elementlerin molleri farklı kütlelere sahiptir, ancak her zaman aynı sayıda atom içerir. Bir elementin bir molünün gram cinsinden kütlesine, mol başına gram cinsinden ifade edilen molar kütle denir.Değeri sayısal olarak elementin atom kütlesine eşittir. Bu nedenle, mol tanımı, parçacıkları tartarak saymamızı sağlar. Molar kütle ve Avogadro sayısı dönüştürme faktörleri olarak kullanılabilir.Bu, 5 gramlık bir altın parçasındaki atom sayısını hesaplamak için kullanılabilir. Altının ortalama molar kütlesi mol başına 196, 96 gramdır. Öyleyse, kütleyi mole dönüştürmek için, altın parçasının kütlesini ortalama molar kütleye bölebiliriz.Ardından, örnekteki toplam atom sayısını elde etmek için mol sayısını Avogadro sayısıyla çarpalım. Yani bu altın külçesi 1, 529 X 10^22 atom içerir.

molar kütle

Bir maddenin kimliği sadece içerdiği atom veya iyon türleri ile değil, aynı zamanda her bir atom veya iyon türünün miktarı ile de tanımlanır. Örneğin, su, H2O ve hidrojen peroksit, H2O2, kendi moleküllerinin hidrojen ve oksijen atomlarından oluşması bakımından benzerdir. Bununla birlikte, bir hidrojen peroksit molekülü, bir oksijen içeren su molekülünün aksine iki oksijen atomu içerdiğinden, iki madde çok farklı özellikler sergiler.
 
 Atomlar ve moleküller son derece küçüktür. Bu nedenle, makroskopik miktarlarını ölçmek için standart bir bilimsel birime ihtiyaç vardır. Mol terimi, çift, düzine, brüt vb. gibi tanıdık birimlere benzer bir miktar birimidir. Bir madde örneğindeki atomların veya moleküllerin sayısının belirli bir ölçüsünü anlatır. "Mol" kelimesinin Latince anlamı, bu birimin adı olarak kullanımıyla tutarlı olan "büyük kütle" veya "toplu"dur. Mol, kolayca ölçülen makroskopik özellik, toplam kütle ve son derece önemli bir temel özellik olan atom sayısı, moleküller vb. arasında bir bağlantı sağlar.
 
 Bir mol maddede 6,02214076 × 1023 adet farklı bileşen (atom ya da molekül) vardır. Bu büyük sayı geleneksel olarak 6,022 × 1023'e yuvarlanır ve İtalyan bilim insanı Amedeo Avogadro anısına Avagadro sayısı (NA) ya da Avagadro sabiti olarak isimlendirilir. Bu sabit raporlama sırasında "mol başına" şeklinde kullanılır.
 
 Bir miktar birimi olarak tanımıyla tutarlı olarak, herhangi bir elementin 1 molü, başka bir elementin 1 molü ile aynı sayıda atom içerir. Bununla birlikte, farklı elementlerin 1 mol kütleleri farklıdır, çünkü bireysel atomların kütleleri büyük ölçüde farklıdır. Bir elementin (veya bileşiğin) molar kütlesi, bu maddenin 1 molünün gram cinsinden kütlesidir, mol başına gram cinsinden ifade edilen bir özelliktir (g/mol).
 
 Herhangi bir maddenin molar kütlesi, amu'daki atomik veya formül ağırlığına sayısal olarak eşdeğerdir. Amu tanımına göre, tek bir karbon atomu 12 amu ağırlığındadır (atomik kütlesi 12 amu'dur). Bir karbon molü 12 g ağırlığındadır (12 g C = 1 mol C atomu = 6,022 × 1023 C atomu) ve karbonun molar kütlesi 12 g/mol'dür. Bu ilişki tüm elementler için geçerlidir, çünkü atomik kütleleri amu referans maddesi karbon-12'ye göre ölçülür. Bu prensibi genişletirsek, bir bileşiğin gram cinsinden molar kütlesi, amu'daki formül kütlesine sayısal olarak eşdeğerdir. Örneğin, helyum 4,002 amu atomik bir kütleye ve 4,002 g/mol molar kütleye sahiptir.
 
 Atomik kütle ve molar kütle sayısal olarak eşdeğer olsa da, ölçek açısından çok farklı olduklarını unutmayın. Molar büyüklüğü anlamak için, yaklaşık 0,03 g ağırlığında küçük bir su damlası düşünün. Bu, 1 mol suyun (~18 g) sadece küçük bir kısmını temsil etse de, hayal edilenden daha fazla su molekülü içerir. Moleküller dünyadaki yaklaşık yedi milyar insan arasında eşit olarak dağıtılsaydı, her insana 100 milyardan fazla su molekülü düşerdi.
 
 Mol, kütle ve atom sayısı arasındaki ilişkiyi tanımlar. Bu, dönüşüm faktörünün uygun formları kullanılarak atom sayısının hesaplanmasına izin verir: 1 mol atom = 6,022 × 1023 atom. Bir elementin kütlesi (gram cinsinden) ile mol sayısı arasında dönüşüm yapmak için, elementin molar kütlesi (g/mol) dönüşüm faktörü olarak kullanılır.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/3-1-formula-mass-and-the-mole-concept"">Openstax Chemistry 2e, Section 3.1: Formula Mass and the Mole Concept.</a>

Molar Kütle

Bir maddenin kimliği, yalnızca içerdiği atom veya iyon türleriyle değil, her bir atom veya iyon türünün miktarıyla da tanımlanır. Mesela...

Education

JoVE Core

Kimya

Atoms and Elements

Atomlar ve Elementler

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

mole, mass, and avogadro’s number

The mole links mass and the number of particles in a substance. It gives chemists a standard way to count atoms and molecules in samples that are far too small to see. It also helps show why substances with the same kinds of atoms can still have very different properties, like water, H2O, and hydrogen peroxide, H2O2.

The mole is an amount unit, like a pair or a dozen. One mole contains 6.02214076 × 10^23 discrete entities, such as atoms or molecules. This number is usually rounded to 6.022 × 10^23 and is called Avogadro’s number, or the Avogadro constant, named for Amedeo Avogadro. The constant is written with the unit per mole.

One mole of any element contains the same number of atoms as one mole of any other element. The masses are different, though, because atoms have different individual masses. That is why one mole of one element does not weigh the same as one mole of another element.

Molar mass is the mass in grams of one mole of a substance. It is reported in grams per mole, or g/mol. The molar mass of an element or compound is numerically equal to its atomic mass or formula mass in amu. For example, carbon has an atomic mass of 12 amu, so 1 mole of carbon has a mass of 12 g and a molar mass of 12 g/mol.

This same relationship works for other elements and for compounds. Helium, for example, has an atomic mass of 4.002 amu and a molar mass of 4.002 g/mol. Although the numbers match, atomic mass and molar mass are very different in scale.

A tiny drop of water can still contain an enormous number of molecules. A drop that weighs about 0.03 g is only a small part of 1 mole of water, which is about 18 g. Even so, it holds more water molecules than can easily be imagined. If those molecules were shared equally among the roughly seven billion people on Earth, each person would still get more than 100 billion molecules of water.

The mole also lets scientists convert between mass and amount. Using the relationship 1 mole of atoms = 6.022 × 10^23 atoms, the number of atoms can be calculated from a sample. The molar mass of an element is also used as a conversion factor to move between grams and moles.

Mole, Mass, and Avogadro’s Number

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molar mass

The mole links mass and the number of particles in a substance. It gives chemists a standard way to count atoms and molecules in samples that are far too small to see. It also helps show why substances with the same kinds of atoms can still have very different properties, like water, H2O, and hydrogen peroxide, H2O2. The mole is an amount unit, like a pair or a dozen. One mole contains 6.02214076 × 10^23 discrete entities, such as atoms or molecules. This number is usually rounded to 6.022 ×...

key terms and concepts

Learn how the mole connects mass, atoms, and molecules through Avogadro’s number and molar mass, with clear examples for high school chemistry.

Mole, Mass, and Avogadro’s Number | JoVE K12

chemistry

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Ohio’s Learning Standards and Model Curriculum

Structure And Properties Of Matter

Quantifying matter

Interactions Of Matter

Stoichiometry

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.a

CH.4

CH.4.a

Physical Science

PS.4

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Arizona Science Standards

High School

HS+C.P1

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Texas Essential Knowledge and Skills

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CHEM.11

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Alabama Course of Study Science

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Florida Department of Education

SC.912.P.8

SC.912.P.8.9

Chemistry and Physics

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Georgia Standards of Excellence

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The Mole Concept and Avogadro’s Number

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Mole, Mass, and Avogadro’s Number

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