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CAIE IGCSE Chemistry 3.2.3 Reacting masses in simple proportions

Practise using balanced equations and simple mass ratios to predict product or reactant masses without using the mole concept.

Syllabus
2026–2028
Course
Chemistry 0620

Exam points

  • use formula masses and equation ratios to calculate masses in carbonate decompositions
  • find a product mass from a given reactant mass in reactions
  • account for incomplete decomposition when calculating the final mass left in a test-tube

3.2.3—Reacting masses in simple proportions question 1

[Maximum number: 1]

The equation for the reaction between hydrogen sulfide, H2 S\mathrm{H}_{2} \mathrm{~S}, and oxygen is shown.

2H2 S+3O2→2SO2+2H2O2 \mathrm{H}_{2} \mathrm{~S}+3 \mathrm{O}_{2} \rightarrow 2 \mathrm{SO}_{2}+2 \mathrm{H}_{2} \mathrm{O}

Which mass of oxygen is required to react with 5.1 g of hydrogen sulfide?

A

2.4 g2.4 \mathrm{~g}

B

4.8 g4.8 \mathrm{~g}

C

7.2 g7.2 \mathrm{~g}

D

14.4 g14.4 \mathrm{~g}

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