The mass of the product is equal to the total mass of the reactants. This is:
Law of conservation of mass
Law of constant proportion
Law of relative mass
Law of reciprocal proportion
The sum of the relative atomic masses of the elements present in a formula unit is:
Relative atomic mass
Relative molecular mass
Relative gram atomic weight
Relative formula mass
The average mass of the naturally occurring atoms of the element, using a scale where an atom of carbon-12 has a mass of exactly 12.
Atomic mass
Molecular mass
Gram atomic mass
The change on one mole of electrons is:
IC
96500 coulombs
600 c
2c
The Faraday constant is:
96500 c/mol
6.023×1023 mol
9.4 × 1021 kg
1.0008 g
Avogadro constant is:
6.02 × 1023
6.02 × 1028
7.1 × 10-31
6.02
The substance which is in large quantity in a solution is called:
Solute
Salt
Precipitate
Solvent
The simplest whole number formula of a compound is:
molecular formula
empirical formula
atomic formula
chemical formula
The mass of on mole of carbon atom.
12 g
56g
2g
100g
The mass of one hydrogen atom is:
1. 6 ×-10-31
1.7 × 10-24
6. 1 × 1023
2.1 × 10-28
