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5070/42

Chemistry 5070/42 — May/June 2013

Cambridge O-Level · Alternative to Practical · worked solutions for every part, with the mark scheme

10
questions
60
marks
60
minutes

Topics Experimental Contexts · Analysis, Conclusions and Evaluation · Observations and Measurements · Use of Techniques, Apparatus and Materials · Qualitative Analysis

Q18MExperimental ContextsObservations and MeasurementsAnalysis, Conclusions and EvaluationFree sample

Iron(II) sulfate crystals have the formula FeSO4⋅xH2O\text{FeSO}_4\cdot x\text{H}_2\text{O}, where xx is a whole number. A student is asked to find the value of xx.

The crystals are placed in a previously weighed crucible which is then reweighed.

(a)

What colour are iron(II) sulfate crystals?

______

1M
(b)

Mass of crucible + iron(II) sulfate crystals = 9.01 g
Mass of crucible = 5.97 g

Calculate the mass of iron(II) sulfate crystals used in the experiment.

______ g\text{g}

1M
(c)

The crystals are gently heated until no more water is given off.
The crucible and contents are cooled and reweighed.

Mass of crucible and iron(II) sulfate after heating = 7.66 g

(i)

Calculate the mass of iron(II) sulfate which remains after heating.

______ g\text{g}

1M
(ii)

Calculate the mass of water lost from the crystals.

______ g\text{g}

1M
(iii)

Calculate the number of moles of iron(II) sulfate that remain after heating.
[MrM_r: FeSO4\text{FeSO}_4, 152]

______ moles

1M
(iv)

Calculate the number of moles of water which are lost on heating.
[MrM_r: H2O\text{H}_2\text{O}, 18]

______ moles

1M
(d)
(i)

Using your answers to (c)(iii) and (c)(iv) calculate the number of moles of water combined with one mole of iron(II) sulfate.

______ moles

1M
(ii)

What is the value of xx in the formula FeSO4⋅xH2O\text{FeSO}_4\cdot x\text{H}_2\text{O}?

x=______x = \_\_\_\_\_\_

1M

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