The relative molecular mass of an element or compound is defined as:
(Average mass of one atom) / (1/12 mass of one atom of carbon-12).
(Average mass of one molecule) / (1/12 mass of one atom of carbon-12).
( mass of one molecule) / (1/12 mass of one atom of carbon-12).
(Average mass of one molecule) / (1/12 mass of one atom of carbon).
At s.t.p, molar volume is:
A. 22400 cm³
B. 22.4 dm³
C. 24000 cm³
ABC.
BC.
AB.
AC.
The definition of the mole is:
The number of molecules in exactly 2 g of hydrogen at room temperature and pressure.
The number of atoms in exactly 12 g of the carbon-12 isotope.
The amount of any substance containing the same number of identical entities as there are carbon atoms in exactly 12 g of the carbon-12 isotope.
The amount of any substance which occupies a volume of 24 dm3 at room temperature and pressure.
The relative atomic mass is defined as:
The mass of an atom of an element relative to the mass of a hydrogen atom.
The average mass of an element relative to 1/12 the mass of a carbon atom.
The average mass of an atom of an element relative to 1/12 the mass of a carbon-12 atom.
The mass of an atom of an element relative to 1/12 the mass of a carbon-12 atom.
