Mole Concept and Molar Mass in Chemistry

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35 Terms

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Mole

The mole, denoted as (mol), is the SI unit representing the amount of substance.

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One mole

One mole is the amount of substance which contains the same number of particles as 12.0 g of Carbon-12.

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Avogadro's number

Avogadro's number, also known as the Avogadro constant is the number of particles in one mole of any substance.

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Avogadro's Number (NA)

NA = 6.022 x 1023

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Molar Mass

The mass of one mole of substance is called the molar mass (or molecular weight). The unit of molar mass is g/mol.

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Mole Ratio

A mole ratio is a conversion factor that relates the number of moles of different substances in a balanced chemical equation.

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Conversion between mole and Avogadro's number

3 moles of HCl contain ................... HCl molecules.

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Moles in atoms of Zinc

How many moles are in 3.01 x 1023 atoms of Zinc?

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Molecules in water

How many molecules do 2.5 moles of water contain?

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Moles of chlorine gas

How many moles of chlorine gas are there in 8.33 x 1023 molecules?

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Molecules in carbon dioxide

How many molecules are in 0.25 mol of carbon dioxide?

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Calculating Molar Mass

To find the molar mass of a compound, you need to sum the atomic masses of all the atoms in the compound, taking into account the number of each atom present.

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Example of Molar Mass Calculation

Calculate molar mass of the following compounds: H₂O, Sodium Carbonate, Potassium Sulfate.

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Stoichiometric relationship

It is a way to express the stoichiometric relationship between reactants and products in a reaction.

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Coefficients in Mole Ratio

To determine the mole ratio, compare the coefficients of each of the substances in the equation.

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Mole Ratio Example

The mole ratio of the above equation is 2 : 1 : 2.

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Mole Ratio of Hydrogen to Water

What is the mole ratio of hydrogen gas to water in the following equation: H2 (g) + O2 (g) H2O (l)?

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Avogadro's constant

The number of particles in one mole of a substance, approximately 6.022 x 10²³.

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Chemical amount in moles

Calculated using the formula n = m / MM, where n is the amount in moles, m is mass in grams, and MM is molar mass in g/mol.

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Percentage composition

The mass percentage of each element within a compound, calculated by dividing the mass of an element by the total mass of the compound and multiplying by 100.

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Molecular formula

A formula that shows the actual number of each type of atom in a molecule.

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Empirical formula

A formula that shows the simplest whole-number ratio of atoms in a compound.

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Calculation of moles

The amount of substance n, in moles, can be calculated for a given mass of substance using the formula n = m / M.

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Example of moles calculation

For 64g of oxygen (O2), n = 64 g / 32.0 g/mol = 2.0 mol O2.

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Percentage composition of sodium carbonate

To determine, divide the mass of sodium by the total mass of sodium carbonate and multiply by 100.

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Percentage composition of Hydrogen in water

Calculated by dividing the mass of Hydrogen in water by the total mass of water and multiplying by 100.

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Example of empirical formula calculation

For a compound with 40% carbon, 6.7% hydrogen, and 53.3% oxygen, the empirical formula is CH2O.

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Steps to calculate empirical formula

1. Convert mass percentages to grams. 2. Convert mass to moles. 3. Divide by the smallest number of moles. 4. Write the empirical formula.

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Example of empirical formula from mass

A compound with 20.32 g of Carbon, 5.12 g of Hydrogen, and 7.9 g of Nitrogen needs to be analyzed to find its empirical formula.

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Mass of sodium chloride

To find the mass of 0.2 mol of sodium chloride, multiply the number of moles by the molar mass of sodium chloride.

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Finding moles of potassium bromide

Calculate the number of moles in 2.48 g of potassium bromide using the formula n = m / M.

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Finding moles of carbonate

Calculate the number of moles in 6 kg of carbonate using the formula n = m / M.

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Finding moles of hydrogen

Calculate the number of moles in 10 g of hydrogen using the formula n = m / M.

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Diatomic molecule

A molecule composed of two atoms, such as O2.

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Mass of glucose sample

To find the number of moles in a 1.52 kg sample of glucose C₆H₁₂O₆, convert kg to g and use the formula n = m / M.