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MATTER - PROPERTIES AND TRANSFORMATION: Chemistry Of Elements - Alkali metals and alkaline earth metals
MATTER - PROPERTIES AND TRANSFORMATION: Chemistry Of Elements - Identification Of Ions
MATTER - PROPERTIES AND TRANSFORMATION: Chemistry Of Elements - Salts
MATTER - PROPERTIES AND TRANSFORMATION: Chemistry Of Elements - Transition metals
MATTER - PROPERTIES AND TRANSFORMATION: Chemistry of Elements - Nitrogen
MATTER - PROPERTIES AND TRANSFORMATION: Chemistry of Elements - Sulphur
MATTER - PROPERTIES AND TRANSFORMATION: Organic Chemistry - Hydrocarbons
MATTER - PROPERTIES AND TRANSFORMATION: Principles Of Chemistry - Formulae, Moles And Equations
MATTER - PROPERTIES AND TRANSFORMATION: Principles Of Chemistry - Gaseous State
MATTER: PROPERTIES AND TRANSFORMATION: Principles Of Chemistry - Solutions and acid-base titration
PRINCIPLES OF CHEMISTRY: Electrochemistry

What is the number of moles of calcium carbonate in 20 g of a sample of it?

0.2 mol

0.01 mol

1 mol

0.1 mol

If the empirical formula of a compound is CH₂ and its relative molecular mass is 56, what is its molecular formula? (C=12, H=1)

CH₂.

C₂H₄.

C₃H₆.

C₄H₈.

The number of particles or entities in a given sample of a substance is given by:

Number of particles = Number of moles of particles × molar mass

Number of particles = mass of particles × Avogadro constant

Number of particles = Number of moles of particles × Avogadro constant

Number of particles = Number of atoms of particles × Avogadro constant

The amount of a substance that contains 6.02×10²³ elementary particles or entities’ is:

Gas constant

Molar mass

Avogadro constant

Mole

The relative molecular mass (RMM) 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)