MOLECULAR MASS
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Molecular mass is the sum of the atomic masses of all the atoms in a molecule. Formula unit mass is the sum of atomic masses of all atoms in a formula unit of a compound, such as sodium chloride (NaCl) which has a formula unit mass of 58.5 u. The mole concept refers to one mole being the amount of substance that contains as many elementary entities (atoms, molecules, ions or particles) as there are atoms in exactly 12 grams of carbon-12, where one mole contains 6.022x10^23 elementary entities and the mass in grams of one mole of a substance is equal to its molar mass.
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3) Key concepts covered include the mole as a unit for counting particles, molar mass, and conversion factors involving moles, mass, and number of particles.
The mole concept
The mole is a unit used in chemistry to express amounts of substances. It represents 6.022x10^23 elementary entities, such as atoms, molecules, ions or other particles of a substance. This number is known as Avogadro's constant, after scientist Amedeo Avogadro who proposed that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. The mass of one mole of a substance, known as its molar mass, can be used to determine the number of moles in a given mass of that substance and vice versa through calculation.
2. F.sc chemistry chapter#01 "Stoichiometry"
The uploaded slides are covering the whole chapter of "Stoichiometry" especially related to KPK boards.
Chem.pptx
Stoichiometry is the study of quantitative relationships between amounts of substances involved in chemical reactions. It allows chemists to determine mole and particle quantities. The mole is the standard unit for measuring amounts of substances and refers to 6.022x1023 elementary entities. Molar mass is the mass of one mole of a substance and is calculated differently for elements versus compounds. Percent composition by mass can be determined by dividing the mass of each element by the total molar mass. Empirical and molecular formulas relate the simplest and actual ratios of elements in a compound.
Chemistry - Chp 10 - Chemical Quantities - PowerPoint
This chapter discusses methods for measuring quantities of substances. It introduces the mole as a unit for measuring amounts of matter equal to Avogadro's number of representative particles. The mole allows for easy conversion between mass and number of particles. Compound formulas allow calculating formula mass in grams per mole. Relationships between moles, mass, and volume at standard temperature and pressure enable interconversion between these quantities.
Mole concept
This document discusses the mole concept in chemistry. A mole is the amount of a substance that contains 6.022x1023 elementary entities and can be used to quantify atoms, molecules, ions or other particles. The mass of a mole of a substance is equal to its molar mass in grams. Some examples given are that 1 mole of oxygen is 16 grams, 1 mole of carbon is 12 grams, and 1 mole of iron is 56 grams. The document also notes that Avogadro's number, which is 6.022x1023, is defined as the number of elementary entities in 1 mole of a substance.
Ib quan chemistry(mole concept)
1. The relative formula mass of calcium carbonate (CaCO3) is 100 g/mol.
2. One mole of calcium carbonate will react with 2 moles of hydrochloric acid (HCl).
3. Therefore, the mass of hydrochloric acid that will react with 1 mole (100 g) of calcium carbonate is 2 x 36.5 g = 73 g, since the molar mass of HCl is 36.5 g/mol.
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MOLECULAR MASS
- 1. Molecular mass and mole concept
- 2. WHAT IS MOLECULAR MASS?? MOLECULAR MASS OF A SUBSTANCE IS THE SUM OF THE ATOMIC MASSES OF ALL THE ATOMS IN THE MOLECULE OF THE SUBSTANCE. THEREFORE, THE RELATIVE MASS OF A MOLECULE IS EXPRESSED IN ATOMIC MASS UNITS (u). WHAT IS FORMULA UNIT MASS?? THE FORMULA UNIT MASS OF AS SUBSTANCE IS THE SUM OF THE ATOMIC MASSES OF ALL ATOMS IN A FORMULA UNIT OF A COMPOUND. FOR EXAMPLE, SODIUM CHLORIDE HAS A FORMULA UNIT NaCl. IT’S FORMULA UNIT CAN BE CALCULATED AS- = 1*23+1*35.5=585u THAT IS (no.of Na atoms*u of Na+ no.of Cl atoms*u of Cl)
- 3. WHAT IS THE MOLE CONCEPT?? ONE MOLE OF ANY SPECIES(ATOMS, MOLECULES, IONS OR PARTICLES) IS THAT QUANTITY IN NUMBER HAVING A MASS EQUAL TO ITS ATOMIC OR MOLECULAR MASS IN GRAMS(g). THE NO.OF PARTICLES(ATOMS, MOLECULES OR IONS) PRESENT IN ONE MOLE OF ANY SUBSTANCE IS FIXED, WITH A VALUE OF 6.022*10^23. THIS NUMBER IS CALLED AS THE AVAGRADO CONSTANT OR AVAGRADO NUMBER. TO GET THE MASS OF 1 MOLE OF ATOM OF AN ELEMENT, THAT IS, MOLAR MASS, WE HAVE TO TAKE THE SAME NUMERICAL VALUE BUT CHANGE THE UNITS FROM “u” TO “g”. MOLAR MASS OF AN OBJECT IS ALSO KNOWN AS THE GRAM ATOMIC MASS. Eg:- u OF hydrogen= 1u. SO, g OF hydrogen=1 g. 1u OF hydrogen HAS ONLY 1 ATOM OF hydrogen. 1g OF hydrogen HAS ONLY 1 MOLE OF ATOMS,THAT IS, 6.022*10^23 ATOMS OF hydrogen. CHEMISTS NEED THE NO.OF ATOMS AND MOLECULES WHILE CARRYING OUT REACTIONS, AND NEED TO RELATE MASS IN GRAMS TO THE NUMBER. IT IS DONE AS FOLLOWS: 1 MOLE= 6.022*10^23 NUMBER
- 4. FACTS ABOUT THE MOLE CONCEPT!! THE WORD MOLE WAS INTRODUCED AROUND 1896 BY WILHELM OSTWALD WHO DERIVED THE TERM FROM THE LATIN WORD MOLES MAENING A HEAP OR PILE. THE SUBSTANCE MAY BE CONDIDERED AS A HEAP OF ATOMS OR MOLECULES. THE UNIT MOLE WAS ACCEPTED IN 1967 TO PROVIDE A SIMPLE WAY OF REPORTING A LARGE NUMBER– THE MASSIVE HEAP OF ATOMS AND MOLECULES IN A SAMPLE.