Curriculum
Course: Combined Science 0653 — Chemistry
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Curriculum

Combined Science 0653 — Chemistry

1. Experimental Chemistry

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2. The Particulate Nature of Matter

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3. Formulae, Stoichiometry and the Mole Concept

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4. Electrolysis

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5. Energy from Chemicals

0/6

6. Chemical Reactions

0/21

7. Acids, Bases and Salts

0/16

8. The Periodic Table

0/19

9. Metals

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10. Air and the Environment

0/11

11. Organic Chemistry

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Quiz

3.1 Formulas – Check yourself

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Formulas Combined Science Chemistry check yourself quiz: free practice for Combined Science (chemistry). Work through this Formulas Combined Science Chemistry check yourself quiz and get instant feedback on every answer. If you get stuck, review the 3.1 Formulas — Notes lesson. More practice: Combined Science (chemistry) — all units. Syllabus: Cambridge IGCSE qualifications.

  • Questions count: 7
  • Passing grade: B+
  • Time limit: 10 minutes
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1.
In the sequence covered in this lesson, which step comes immediately after × M?
In the sequence covered in this lesson, which step comes immediately after × M?
÷ M
× ratio
Moles of product
Mass
2.
Which statement best describes Concentration?
Which statement best describes Concentration?
Simplest whole-number ratio of atoms.
24 dm³ mol⁻¹ at r.t.p.
mol dm⁻³ = moles ÷ volume (dm³).
Actual number of atoms of each element.
3.
Which step comes first in the sequence covered in this lesson?
Which step comes first in the sequence covered in this lesson?
Mass
Moles of product
Moles
÷ M
4.
Which key term matches this description: "Actual number of atoms of each element."
Which key term matches this description: "Actual number of atoms of each element."
Limiting reagent
Molecular formula
Relative atomic mass (Ar)
Molar gas volume
5.
Complete the statement: n = ______.
Complete the statement: n = ______.
Limiting reagent
Mole
m ÷ M
Relative atomic mass (Ar)
6.
Which statement best describes Relative atomic mass (Ar)?
Which statement best describes Relative atomic mass (Ar)?
24 dm³ mol⁻¹ at r.t.p.
Weighted mean mass of an atom relative to 1/12 of carbon-12.
Mass of one mole, in g mol⁻¹.
Reactant completely used up first.
7.
According to the comparison table in this lesson, what is the Tip of Moles from solution?
According to the comparison table in this lesson, what is the Tip of Moles from solution?
Key mole calculations
Less than 100% due to losses
R = 8.31 J K⁻¹ mol⁻¹
Convert cm³ ÷ 1000
Higher = less waste
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Part of 3. Formulae, Stoichiometry and the Mole Concept — see every lesson and quiz in this unit.
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