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Mole

ml/noun

1. 1.a small burrowing insectivorous mammal with dark velvety fur, a long muzzle, and verysmall eyes.

2. 2.a spy who achieves over a long period an important position within the securitydefenses of a country.synonyms:spy,agent,secret agent,undercover

agent,operative,plant,infiltrator,sleeper,informant,informer;More

Avogadro's

Avogadro's law(sometimes referred to as Avogadro's hypothesisor Avogadro's principle) is an

experimentalgas law relatingvolume of a gas to theamount of substanceof gas present. A modern

statement of Avogadro's law is:

Avogadro's law states that, "equal volumes of all gases, at the same temperature and pressure,

have the same number of molecules".

For a given mass of anideal gas,the volume and amount (moles) of the gas are directly proportional

if thetemperature andpressure are constant.

which can be written as:

or

where:

Vis thevolume of the gas

nis theamount of substance of the gas (measured inmoles).

kis aconstant equal to RT/P, where R is the universal gas constant, T is the Kelvintemperature, and P is the pressure. As temperature and pressure are constant, RT/P is alsoconstant and represented as k.This is derived from theideal gas law.

This law explains how, under the same condition oftemperature andpressure,

equalvolumes of allgases contain the same number ofmolecules.For

comparing the same substance under two different sets of conditions, the law

can be usefully expressed as follows:
https://www.google.com.ph/search?biw=1366&bih=677&q=define+spy&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CB0Q_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+spy&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CB0Q_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+agent&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CB4Q_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+secret+agent&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CB8Q_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+operative&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCAQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+plant&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCEQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+sleeper&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCIQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+informant&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCMQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+informer&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCQQ_SowAAhttp://en.wikipedia.org/wiki/Amedeo_Avogadrohttp://en.wikipedia.org/wiki/Amedeo_Avogadrohttp://en.wikipedia.org/wiki/Gas_lawshttp://en.wikipedia.org/wiki/Volumehttp://en.wikipedia.org/wiki/Amount_of_substancehttp://en.wikipedia.org/wiki/Ideal_gashttp://en.wikipedia.org/wiki/Temperaturehttp://en.wikipedia.org/wiki/Pressurehttp://en.wikipedia.org/wiki/Volumehttp://en.wikipedia.org/wiki/Amount_of_substancehttp://en.wikipedia.org/wiki/Mole_(unit)http://en.wikipedia.org/wiki/Constant_(mathematics)http://en.wikipedia.org/wiki/Ideal_gas_lawhttp://en.wikipedia.org/wiki/Temperaturehttp://en.wikipedia.org/wiki/Pressurehttp://en.wikipedia.org/wiki/Volumehttp://en.wikipedia.org/wiki/Gashttp://en.wikipedia.org/wiki/Moleculehttp://en.wikipedia.org/wiki/Moleculehttp://en.wikipedia.org/wiki/Gashttp://en.wikipedia.org/wiki/Volumehttp://en.wikipedia.org/wiki/Pressurehttp://en.wikipedia.org/wiki/Temperaturehttp://en.wikipedia.org/wiki/Ideal_gas_lawhttp://en.wikipedia.org/wiki/Constant_(mathematics)http://en.wikipedia.org/wiki/Mole_(unit)http://en.wikipedia.org/wiki/Amount_of_substancehttp://en.wikipedia.org/wiki/Volumehttp://en.wikipedia.org/wiki/Pressurehttp://en.wikipedia.org/wiki/Temperaturehttp://en.wikipedia.org/wiki/Ideal_gashttp://en.wikipedia.org/wiki/Amount_of_substancehttp://en.wikipedia.org/wiki/Volumehttp://en.wikipedia.org/wiki/Gas_lawshttp://en.wikipedia.org/wiki/Amedeo_Avogadrohttp://en.wikipedia.org/wiki/Amedeo_Avogadrohttps://www.google.com.ph/search?biw=1366&bih=677&q=define+informer&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCQQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+informant&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCMQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+sleeper&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCIQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+plant&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCEQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+operative&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CCAQ_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+secret+agent&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CB8Q_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+agent&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CB4Q_SowAAhttps://www.google.com.ph/search?biw=1366&bih=677&q=define+spy&sa=X&ei=GTVfVNLrO6K8mQXil4KwBQ&ved=0CB0Q_SowAA


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The equation shows that, as the number of moles of gas increases, the

volume of the gas also increases in proportion. Similarly, if the number of

moles of gas is decreased, then the volume also decreases. Thus, the

number of molecules or atoms in a specific volume of idealgas is

independent of their size or themolar mass of the gas.

The law is named afterAmedeo Avogadro who, in 1811,[1]hypothesized

that two given samples of an ideal gas, of the same volume and at the

same temperature and pressure, contain the same number of molecules.

As an example, equal volumes of molecularhydrogen andnitrogen contain

the same number of molecules when they are at the same temperature and

pressure, and observeideal gas behavior. In practice, real gases show

small deviations from the ideal behavior and the law holds only

approximately, but is still a useful approximation for scientists.

Molar masses of elements

Main article:Relative atomic mass

The molar mass ofatoms of anelement is given by theatomic mass of the element[2]multiplied by

themolar mass constant,M

u= 1103kg/mol = 1 g/mol:[3]M(H) = 1.007 97(7) 1 g/mol = 1.007 97(7) g/mol

M(S) = 32.065(5) 1 g/mol = 32.065(5) g/mol

M(Cl) = 35.453(2) 1 g/mol = 35.453(2) g/mol

M(Fe) = 55.845(2) 1 g/mol = 55.845(2) g/mol.

Multiplying by the molar mass constant ensures that the calculation

isdimensionally correct: atomic weights are dimensionless quantities (i.e., pure

numbers) whereas molar masses have units (in this case, grams/mole).

Some elements are usually encountered asmolecules,e.g.hydrogen (H

2),sulfur (S

8),chlorine (Cl

2). The molar mass of molecules of these elements is the molar mass of the atoms

multiplied by the number of atoms in each molecule:M(H2) = 2 1.007 97(7) 1 g/mol = 2.015 88(14) g/molM(S8) = 8 32.065(5) 1 g/mol = 256.52(4) g/molM(Cl2) = 2 35.453(2) 1 g/mol = 70.906(4) g/mol.

Molar masses of compounds

The molar mass of acompound is given by the sum of thestandard

atomic mass of theatoms which form the compound multiplied by
http://en.wikipedia.org/wiki/Gashttp://en.wikipedia.org/wiki/Molar_masshttp://en.wikipedia.org/wiki/Amedeo_Avogadrohttp://en.wikipedia.org/wiki/Avogadro's_law#cite_note-1http://en.wikipedia.org/wiki/Avogadro's_law#cite_note-1http://en.wikipedia.org/wiki/Avogadro's_law#cite_note-1http://en.wikipedia.org/wiki/Hydrogenhttp://en.wikipedia.org/wiki/Nitrogenhttp://en.wikipedia.org/wiki/Ideal_gashttp://en.wikipedia.org/wiki/Relative_atomic_masshttp://en.wikipedia.org/wiki/Atomhttp://en.wikipedia.org/wiki/Chemical_elementhttp://en.wikipedia.org/wiki/Atomic_masshttp://en.wikipedia.org/wiki/Molar_mass#cite_note-AtWt-2http://en.wikipedia.org/wiki/Molar_mass#cite_note-AtWt-2http://en.wikipedia.org/wiki/Molar_mass#cite_note-AtWt-2http://en.wikipedia.org/wiki/Molar_mass_constanthttp://en.wikipedia.org/wiki/Molar_mass#cite_note-CODATA2010-3http://en.wikipedia.org/wiki/Molar_mass#cite_note-CODATA2010-3http://en.wikipedia.org/wiki/Molar_mass#cite_note-CODATA2010-3http://en.wikipedia.org/wiki/Dimensionhttp://en.wikipedia.org/wiki/Moleculehttp://en.wikipedia.org/wiki/Hydrogenhttp://en.wikipedia.org/wiki/Sulfurhttp://en.wikipedia.org/wiki/Chlorinehttp://en.wikipedia.org/wiki/Chemical_compoundhttp://en.wikipedia.org/w/index.php?title=Standard_atomic_mass&action=edit&redlink=1http://en.wikipedia.org/w/index.php?title=Standard_atomic_mass&action=edit&redlink=1http://en.wikipedia.org/wiki/Atomhttp://en.wikipedia.org/wiki/Atomhttp://en.wikipedia.org/w/index.php?title=Standard_atomic_mass&action=edit&redlink=1http://en.wikipedia.org/w/index.php?title=Standard_atomic_mass&action=edit&redlink=1http://en.wikipedia.org/wiki/Chemical_compoundhttp://en.wikipedia.org/wiki/Chlorinehttp://en.wikipedia.org/wiki/Sulfurhttp://en.wikipedia.org/wiki/Hydrogenhttp://en.wikipedia.org/wiki/Moleculehttp://en.wikipedia.org/wiki/Dimensionhttp://en.wikipedia.org/wiki/Molar_mass#cite_note-CODATA2010-3http://en.wikipedia.org/wiki/Molar_mass_constanthttp://en.wikipedia.org/wiki/Molar_mass#cite_note-AtWt-2http://en.wikipedia.org/wiki/Atomic_masshttp://en.wikipedia.org/wiki/Chemical_elementhttp://en.wikipedia.org/wiki/Atomhttp://en.wikipedia.org/wiki/Relative_atomic_masshttp://en.wikipedia.org/wiki/Ideal_gashttp://en.wikipedia.org/wiki/Nitrogenhttp://en.wikipedia.org/wiki/Hydrogenhttp://en.wikipedia.org/wiki/Avogadro's_law#cite_note-1http://en.wikipedia.org/wiki/Amedeo_Avogadrohttp://en.wikipedia.org/wiki/Molar_masshttp://en.wikipedia.org/wiki/Gas


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themolar mass constant,M

u:M(NaCl) = [22.989 769 28(2) + 35.453(2)] 1 g/mol = 58.443(2) g/mol

M(C12H

22O11) = ([12 12.0107(8)] + [22 1.007 94(7)] + [11 15.9994(3)]) 1 g/mol =342.297(14) g/mol.

An average molar mass may be defined for mixtures of

compounds.[1]This is particularly important inpolymer science,

where different polymer molecules may contain different

numbers ofmonomer units (non-uniform polymers).[4][5]

Average molar mass of mixtures

The average molar mass of mixtures can be calculatedfrom themole fractions of the components and their molar

masses :

It can also be calculated from themass fractions of the

components:

As an example, the average molar mass of dry air is

28.97 g/mol.[6]

Formula Mass Definition: The formula mass of a molecule is the sum of the atomic weights of

the atoms in the empirical formula of the compound.

Also Known As: formula weight

Examples: The molecular formula for glucose is C6H12O6, so the empirical formula is CH2O.

The formula mass of glucose is (12)+2(1)+16 = 30 amu.

Calculating formula masses

Since a molecule - scratch that, there we go again, calling everything molecules! Since a formula is made

of atoms, we can calculate a formula mass by simply adding up all the atoms that are in it. This is an

application of the law of conservation of mass. Count up the number of atoms of each type in the

formula, and add up the total mass. We've broken this out in the form of a table in these examples, and

you'll probably want to use a somewhat similar method.

Which of the following is a correct calculation of the formula mass?
http://en.wikipedia.org/wiki/Molar_mass_constanthttp://en.wikipedia.org/wiki/Molar_mass#cite_note-GreenBook-1http://en.wikipedia.org/wiki/Molar_mass#cite_note-GreenBook-1http://en.wikipedia.org/wiki/Molar_mass#cite_note-GreenBook-1http://en.wikipedia.org/wiki/Polymer_sciencehttp://en.wikipedia.org/wiki/Monomerhttp://en.wikipedia.org/wiki/Molar_mass#cite_note-4http://en.wikipedia.org/wiki/Molar_mass#cite_note-4http://en.wikipedia.org/wiki/Molar_mass#cite_note-4http://en.wikipedia.org/wiki/Mole_fractionhttp://en.wikipedia.org/wiki/Mass_fraction_(chemistry)http://en.wikipedia.org/wiki/Molar_mass#cite_note-6http://en.wikipedia.org/wiki/Molar_mass#cite_note-6http://en.wikipedia.org/wiki/Molar_mass#cite_note-6http://en.wikipedia.org/wiki/Mass_fraction_(chemistry)http://en.wikipedia.org/wiki/Mole_fractionhttp://en.wikipedia.org/wiki/Molar_mass#cite_note-4http://en.wikipedia.org/wiki/Molar_mass#cite_note-4http://en.wikipedia.org/wiki/Monomerhttp://en.wikipedia.org/wiki/Polymer_sciencehttp://en.wikipedia.org/wiki/Molar_mass#cite_note-GreenBook-1http://en.wikipedia.org/wiki/Molar_mass_constant


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Na2CO3

39.12 NH4Cl

25.00 BaSO4

233.4 None of these

What is the formula mass of CaCO3 to 1 decimal place?

When a formula contains polyatomic ions, the number of atoms inside the brackets are multiplied by

any subscript immediately behind the brackets, as shown in this example.

Here's another polyatomic ion example.


Ca(OH)2

114.16 (NH4)2CO3

80.00 Al2(SO4)3

278.1 None of these

What is the formula mass of Ba(HSO3)2 to 1 decimal place?

Sometimes when ionic crystals form, water becomes a part of the crystal structure. This is known as

water of hydration, and the crystals are called "hydrates", or "hydrated salts". Formulas for hydrates

always include a dot separator, followed by the number of water molecules attached, such as formulas

like CuSO4.5H2O. There are several ways you can do such formulas. One method is to treat the water of

hydration as having its own mass, and add it to the other masses as shown in this example.


FeCl2.4H2O

198.75 AlCl3.6H2O

818.1 Na2CO3.10H2O

180.00 MgSO4.7H2O

120.37

The above were all examples of ionic formulas, but exactly the same principle applies to true molecular

formulas, such as that of glucose.

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