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3.2 Use of amount of substance in relation to masses of pure substances

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Question 36
H

2.4 g of carbon reacts completely with 3.2 g of oxygen to produce 5.6 g of carbon monoxide.

Relative atomic masses (ArA_rAr​): C=12\text{C} = 12C=12, O=16\text{O} = 16O=16

Which equation for this reaction is balanced correctly?

[1]
A

C+O2→CO2\text{C} + \text{O}_2 \rightarrow \text{CO}_2C+O2​→CO2​

B

2C+O2→2CO2\text{C} + \text{O}_2 \rightarrow 2\text{CO}2C+O2​→2CO

C

C+2O2→CO4\text{C} + 2\text{O}_2 \rightarrow \text{CO}_4C+2O2​→CO4​

D

2C+2O2→2CO22\text{C} + 2\text{O}_2 \rightarrow 2\text{CO}_22C+2O2​→2CO2​

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3.2 Use of amount of substance in relation to masses of pure substances Questions

  1. GCSE
  2. /Chemistry
  3. /3.2 Use of amount of substance in relation to masses of pure substances

131 exam-style questions on AQA GCSE Chemistry 3.2 Use of amount of substance in relation to masses of pure substances, covering 3.2.1 Moles, 3.2.2 Amounts of substances in equations, 3.2.3 Using moles to balance equations, 3.2.4 Limiting reactants, 3.2.5a Concentration of solutions, and 3.2.5b Relating mass, volume and concentration. Each one has a worked solution and a mark scheme showing where the marks go.

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