5. Explain
A. The need of the term average atomic
mass.
B. Molar mass.
C. Mole concept.
D. Formula mass with an example.
E. Molar volume of gas.
F. Types of matter (on the basis of chemical
composition).
Answers
Answer:
A)Several naturally occurring elements exist as a mixture of two or more isotopes. ... For this purpose, the atomic masses of isotopes and their relative percentage abundances are considered. Hence, the term average atomic mass is needed to express the atomic mass of elements containing a mixture of two or more isotopes.
B)The molar mass of a chemical compound is defined as the mass of a sample of that compound divided by the amount of substance in that sample, measured in moles. The molar mass is a bulk, not molecular, property of a substance.
C)A mole is defined as the amount of substance containing the same number of discrete entities (atoms, molecules, ions, etc.) ... The molar mass of an element (or compound) is the mass in grams of 1 mole of that substance, a property expressed in units of grams per mole (g/mol)
D)Mass of k atoms(g)/Devide Molar Mass(g/mol)→Moll of k atoms(mol)
ex:The formula mass of a molecule (also known as formula weight) is the sum of the atomic weights of the atoms in the empirical formula of the compound. Formula weight is given in atomic mass units (amu)
Multiply the volume and density together.
Multiply your two numbers together, and you'll know the mass of your object.
E)The molar volume is the volume occupied by one mole of any gas, at room temperature and pressure. The molar volume is equal to 24 dm 3 (24,000 cm 3). This volume is given in questions that need it.
F)On the basis of chemical properties, matter is classified as elements, compounds and mixtures. Solids- Solids have strong molecular force and a definite shape and size solids can neither flow nor be compressed. Liquids- Liquids have weak intermolecular flow and large intermolecular spaces.
Answer:
The atomic mass of such an element is the average of atomic masses of its isotopes. For this purpose, the atomic masses of isotopes and their relative percentage abundances are considered. Hence, the term average atomic mass is needed to express the atomic mass of elements containing a mixture of two or more isotopes.