# H2O Molar Mass

Come friends, today we will know how much H2O Molar Mass is. One of the basic units in the International System of Units (SI) is the mole. So friends, we will go from the beginning about molar mass H2O

Insect – This is the amount of substance that contains as many structural units of a given substance (molecules, atoms, ions, etc.), as there are carbon atoms in 0.012 kg (12 g) of a carbon isotope. 12 together .

Given that the value of the absolute atomic mass for carbon is M (C) = 1.99 10 26 kg, you can calculate the number of carbon atoms N is contained in 0.012 kg of carbon .

One mole of any substance contains the same number of particles of this substance (structural unit). The number of structural units contained in a substance in the volume of one mole is 6.02 10 . is 23 and called Avogadro’s number ( na ).

For example, one mole of copper contains 6.02 10 23 atoms of copper (Cu), and one mole of hydrogen (H2) contains 6.02 10 23 hydrogen molecules.

The molar mass (m) is the mass of a substance taken in an amount of 1 mol.

The molar mass is denoted by the letter M and has the dimension [g/mol]. In physics, the dimension [kg/kmol] is used.

In general, the numerical value of the molar mass of a substance numerically coincides with the value of its relative molecular (relative atomic) mass.

For example, the relative molecular weight of water is:

r (Н 2 ) = 2Аr (Н) + r (O) = 2 1 + 16 = 18 amu

The molar mass of water (H2O) has the same value, but is expressed in g/mol:

M (H 2 O) 18 g / mol.

Thus, one mole of water containing 6.02 10 23 water molecules (2 6.02 10 23 hydrogen atoms and 6.02 10 23 oxygen atoms, respectively) has a mass of 18 grams. The amount of matter in water is 1 mol, it contains 2 mol of hydrogen atoms and one mol of oxygen atoms.

## RELATIONSHIP BETWEEN MASS OF A SUBSTANCE AND ITS VOLUME

Knowing the mass of a substance and its chemical formula and hence the value of its molar mass, it is possible to determine the amount of a substance and, conversely, by knowing the amount of a substance it is possible to determine its mass. For such calculations, you should use the formulas:

where is the amount of substance, [mol]; m – mass of the substance, [g] or [kg]; M is the molar mass of the substance, [g / mol] or [kg / kmol].

For example, to find the mass of sodium sulfate (Na 2 SO 4) in an amount of 5 mol, we get:

1) The value of the relative molecular weight of Na 2 SO 4, which is the sum of the rounded values ​​of the relative atomic mass:

r (Na 2 SO 4) = 2Аr (Na) + r (S) + 4Аr (O) = 142,

2) the numerically equal value of the molar mass of the substance:

M (Na 2 SO 4) 142 g / mol,

3) And, finally, the mass of 5 mol sodium sulfate:

M = M 5 mol 142 g / mol = 710 g.

## RELATIONSHIP BETWEEN THE VOLUME OF A SUBSTANCE AND ITS QUANTITY

Under normal circumstances (number), ie. At a pressure R equal to 101325 Pa (760 mm Hg), and a temperature T, equal to 273.15 K (0), one mole of different gases and vapors in the same volume, equal 22.4 L.

The volume occupied by 1 mole of gas or vapor under normal conditions is called the molar volume of the gas and has a dimension of liter per mole.

V mol = 22.4 L / mol.

Knowing the amount of a gaseous substance (ν ) and the molar volume value (V mol) you can calculate its volume (V) under normal conditions:

V = V mol,

where is the amount of substance [mol]; V is the volume of the gaseous substance [L]; V mol = 22.4 L / mol.

And, conversely, knowing the volume ( V ) of the gaseous substance under normal conditions, you can calculate its volume (ν) :

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### Chemical formula

Molar mass of H2O, water 18.01528 g / mol

1.00794 2 + 15.9994

### MASS FRACTION OF ELEMENTS IN A COMPOUND

Using the Molar Mass Calculator

• Chemical formulas should be filed case sensitive
• Indexes are entered as regular numbers
• For example, the point at the midline (multiplication sign) used in formulas for crystalline hydrates is replaced by a simple dot.
• Example: Instead of CuSO₄ 5H₂O, the converter uses the CuSO4.5H2O spelling for ease of input.

## MOLAR MASS CALCULATOR

### INSECT

All matter is made up of atoms and molecules. In chemistry, it is important to accurately measure the mass of substances that react and obtain results from it. By definition, mole is the SI unit of quantity of a substance. There are exactly 6.02214076 × 10²³ elementary particles in one mole. This value is numerically equal to the Avogadro constant NA, if it is expressed in units of mol and is called the Avogadro number. The amount of matter (symbol n ) is a measure of the number of structural elements of the system. A building block can be an atom, molecule, ion, electron, or any particle or group of particles.

Avogadro’s constant NA = 6.02214076 × 10²³ mol⁻¹. Avogadro’s number is 6.02214076 × 10²³.

In other words, one mole is equal to the mass of a substance equal to the sum of the atomic masses of the atoms and molecules of a substance, multiplied by Avogadro’s number. The mol, the unit of quantity of a substance, is one of the seven basic units of the SI system and is denoted by the mol. Since the name of the entity and its symbol coincide, it should be noted that the symbol is not rejected, unlike the name of the entity, which can be rejected according to the general rules of the Russian language. One mole of pure carbon-12 is exactly 12 grams.

## MOLAR MASS, H2O

Molar mass is a physical property of a substance, defined as the ratio of the amount of substance in moles to the mass of this substance. In other words, it is the mass of one mole of a substance. The unit of molar mass in SI is kg/mol (kg/mol). However, chemists are used to using the more convenient unit of g/mol.

molar mass = g / mole

### MOLAR MASS OF ELEMENTS AND COMPOUNDS

Compounds – substances consisting of different atoms that are chemically related to each other. For example, the following substances, which can be found in the kitchen of any housewife, are chemical compounds:

• Salt (sodium chloride) NaCl
• Sugar (Sucrose) C₁₂H₂₂O₁₁
• Vinegar (acetic acid solution) CH₃COOH

The molar mass of chemical elements in grams per mole numerically coincides with the mass of the element’s atoms, expressed in atomic mass units (or daltons). The molar mass of a compound is equal to the sum of the molar masses of the elements that make up the compound, taking into account the number of atoms in the compound. For example, the molar mass of H2O water is approximately 1 × 2 + 16 = 18 g/mol.

### MOLECULAR MASS

Molecular weight (formerly called molecular weight) is the mass of a molecule, calculated as the sum of the masses of each atom multiplied by the number of atoms in that molecule. Molecular weight is a dimensionless physical quantity, numerically equal to the molar mass. That is, the molecular weight differs from the molar weight in dimension. Despite the fact that molecular weight is a dimensionless quantity, it still has a quantity called an atomic mass unit (emu) or dalton (Da), and a mass approximately equal to that of a proton or neutron. The atomic mass unit is also numerically equal to 1 g/mol.

MOLAR MASS CALCULATION

The molar mass is calculated as follows:

Determination of atomic masses of elements according to the periodic table;
Post a question on TC Terms and you will get an answer within minutes.

Water is the most abundant substance found in nature. It is a thermodynamically stable compound with three . Is able to exist in total states : liquid, solid (ice) and gaseous (water vapor), each of which is determined by temperature and pressure (Figure 1).

Rice. 1. Diagram of water conditions.

The AO curve corresponds to equilibrium in the ice-steam system, the DO to the equilibrium in the supercooled water-steam system, the OC curve to the equilibrium in the water-steam system, and the OB curve to the equilibrium in the ice-water system. All the curves intersect at point O. This point is called the triple point and corresponds to the equilibrium in the ice-water-steam system.

The macro formula of water is H2O. As you know, the molecular weight of a molecule is equal to the sum of the relative atomic masses of the atoms that make up the molecule (the value of relative atomic mass taken from DIMendeleev’s periodic table is rounded off to whole numbers).

Mr(H 2 O) = 2 × Ar(H) + Ar(O);

Mr(H 2 O) = 2 × 1 + 16 = 2 + 16 = 18.

Definition

The molar mass (m) is the mass of 1 mole of a substance.

It is easy to show that the molar mass M and the relative molecular mass M r have the same numerical value, but the first quantity has dimension [M] = g/mol, and the second is dimensionless:

M = N a × M (1 molecule) = N a × m r × 1 amu = (n a × 1 amu) × m r = × m r.

This means that the molar mass of water (H2O) is 18 g/mol. is .

### MASS FRACTION OF ELEMENTS IN A COMPOUND

Using the Molar Mass Calculator

• Chemical formulas should be filed case sensitive
• Indexes are entered as regular numbers
• For example, the point at the midline (multiplication sign) used in formulas for crystalline hydrates is replaced by a simple dot.
• Example: Instead of CuSO₄ 5H₂O, the converter uses the CuSO4.5H2O spelling for ease of input.

## MOLAR MASS OF ELEMENTS AND COMPOUNDS

Compounds are substances made up of different atoms that are chemically bonded to each other. For example, the following substances, which can be found in the kitchen of any housewife, are chemical compounds:

• Salt (sodium chloride) NaCl
• Sugar (Sucrose) C₁₂H₂₂O₁₁
• Vinegar (acetic acid solution) CH₃COOH

The molar mass of chemical elements in grams per mole numerically coincides with the mass of the element’s atoms, expressed in atomic mass units (or daltons). The molar mass of a compound is equal to the sum of the molar masses of the elements that make up the compound, taking into account the number of atoms in the compound. For example, the molar mass of water (H2O) is approximately 1 × 2 + 16 = 18 g/mol.

## MOLECULAR MASS

Molecular weight (formerly called molecular weight) is the mass of a molecule, calculated as the sum of the masses of each atom multiplied by the number of atoms in that molecule. Molecular weight is a dimensionless physical quantity, numerically equal to the molar mass. That is, the molecular weight differs from the molar weight in dimension. Despite the fact that molecular weight is a dimensionless quantity, it still has a quantity called the atomic mass unit (emu) or dalton (Da), and is roughly equal to the mass of a proton or neutron. The atomic mass unit is also numerically equal to 1 g/mol.

## MOLAR MASS CALCULATION

The molar mass is calculated as follows:

• Determination of atomic masses of elements according to the periodic table;
• find the number of atoms of each element in the compound formula;
• Determine the molar mass by multiplying the atomic mass of the elements included in the compound by their number.

For example, let’s calculate the molar mass of acetic acid

it consists of:

• two carbon atoms
• four hydrogen atoms
• two oxygen atoms
• Carbon C = 2 × 12.0107 g/mol = 24.0214 g/mol
• Hydrogen H = 4 × 1.00794 g/mol = 4.03176 g/mol
• Oxygen O = 2 × 15.9994 g/mol = 31.9988 g/mol
• Molar mass = 24.0214 + 4.03176 + 31.9988 = 60.05196 g / mol

Our calculator does just that. You can put acetic acid formula in it and check what happens.

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