(a)[1]
Identify the compound present in limestone.
(b(i))[1]
Describe what you would see if a test-tube containing a small amount of hydrated iron(II) sulfate is heated gently.
(b(ii))[2]
Describe a test for aqueous iron(II) ions. test result
(c(i))[1]
Complete the chemical equation for this reaction. $\text{Fe} + \text{H}_2\text{SO}_4 \rightarrow \text{FeSO}_4 + \ldots$
(c(ii))[1]
Describe how you could remove the excess iron from the mixture formed.
(d(i))[2]
Complete the structure of ethanoic acid so that every atom and every bond is shown.
(d(ii))[1]
Give one observation for the reaction between aqueous ethanoic acid and magnesium.
(e)[3]
Draw a labelled diagram of the apparatus used to separate these different coloured dyes by chromatography.
(f)[3]
Explain these observations in terms of the kinetic particle model.