Masses

What does the following definition describe:

"The simplest whole number ratio of atoms or ions of each element in a substance"

• Relative Formula Mass

• Moles

• Relative Atomic Mass

• Empirical Formula

What does the following definition describe:

"The sum of the relative atomic masses of the atoms or ions in its formula"

• Mole

• Relative Atomic Mass

• Relative Formula Mass

• Empirical Formula

Tags

NGSS.HS-PS1-7

Complete the equation:

Moles = ? / Mr

• Mass (g)

• Volume (ml)

• Concentration (g/mol)

• Avogadros Constant Number

Mass = 1g

Mr = 1

How many moles are there?

• 0.1

• 1

• 10

• 100

What would be the correct Empirical Formula for the following ratio of atoms:

Aluminium Chlorine

1:3

• Al₃Cl

• AlCl₃

• 3AlCl

• Al 3Cl

The relative atomic masses for:

Mg = 24

O = 16

What is relative formula mass for MgO?

• 42

• 48

• 40

• 32

What is the balanced equation for:

Mg + O₂ → MgO

• Mg₂ + O₂ → 2MgO

• 2Mg + O₂ → 2MgO

• Mg + O → MgO

• 2Mg + 2O₂ → 2MgO

Tags

NGSS.HS-PS1-7

What is the reactant in the following equation?
2NaHCO₃  -> Na₂CO₃  +  CO₂  + H₂O

• NaHCO₃
• Na₂CO₃
• CO₂
• H₂O

Which of the following describes the law of conservation of mass?

• In a reaction, atoms are created or destroyed.
• In a reaction, atoms are not lost or made.
• In a reaction, the mass of the product may be more or less than the reactants.
• In a reaction, mass never stays the same.

Tags

NGSS.HS-PS1-7

For the equation:
2H₂ +  O₂ --> 2H₂O
How much H₂O will be produced if we react 4g of H₂ and 32g of O₂?

• 4g
• 32g
• 36g
• 28g

Tags

NGSS.HS-PS1-7