Excess zinc powder is stirred into iron(II) sulfate solution.
Zn(s)+FeSO4(aq)→ZnSO4(aq)+Fe(s) \mathrm{Zn(s) + FeSO_{4}(aq) \rightarrow ZnSO_{4}(aq) + Fe(s)} Zn(s)+FeSO4(aq)→ZnSO4(aq)+Fe(s)When the reaction is complete, the mixture is filtered. All the solid iron and unused zinc are removed. No solution is lost.
| Element | Zn | Fe |
|---|---|---|
| Relative atomic mass (ArA_rAr) | 65.4 | 55.8 |
Compared with the original iron(II) sulfate solution, what happens to the mass of the filtrate?
It decreases, because the solid iron that forms in the reaction is removed from the mixture by filtering.
It decreases, because 65.4 g of zinc leaves the solution for every 55.8 g of iron that goes into it.
It increases, because 65.4 g of zinc goes into the solution for every 55.8 g of iron that leaves it.
It stays the same, because the coefficients for zinc and iron in the equation are equal.
113 exam-style questions on OCR GCSE Chemistry 4.1 Predicting chemical reactions, covering 4.1.1 Properties and trends in Groups 1, 7 and 0, 4.1.2 Properties of the transition metals, 4.1.3 Reactivity predicted from position in the Periodic Table, and 4.1.4 Reactivity of metals and the reactivity series. Each one has a worked solution and a mark scheme showing where the marks go.