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3.1 Introducing chemical reactions

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Question 28
H

0.58 g of a hydrocarbon burns completely in oxygen. It makes 1.76 g of carbon dioxide and 0.90 g of water.

The relative formula mass of the hydrocarbon is 58.0.

Relative atomic mass (ArA_rAr​): H = 1.0 C = 12.0 O = 16.0

What is the molecular formula of the hydrocarbon?

[1]
A

C2H5\mathrm{C_{2}H_{5}}C2​H5​

B

C3H8\mathrm{C_{3}H_{8}}C3​H8​

C

C4H8\mathrm{C_{4}H_{8}}C4​H8​

D

C4H10\mathrm{C_{4}H_{10}}C4​H10​

Markscheme

3.1 Introducing chemical reactions Questions

  1. GCSE
  2. /Chemistry
  3. /3.1 Introducing chemical reactions

55 exam-style questions on OCR GCSE Chemistry 3.1 Introducing chemical reactions, covering 3.1.1 Writing formulae and balanced chemical equations, 3.1.2 Formulae of compounds from ions, and state symbols, 3.1.3 Conservation of mass and observed changes in mass, 3.1.4 Half equations and balanced ionic equations, 3.1.5 The mole and the Avogadro constant, and 3.1.6 Stoichiometry, limiting reactants and reacting masses. Each one has a worked solution and a mark scheme showing where the marks go.

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