A student puts a strip of zinc into copper sulfate solution. Copper forms on the strip.
Zn+CuSO4→ZnSO4+Cu \mathrm{Zn + CuSO_{4} \rightarrow ZnSO_{4} + Cu} Zn+CuSO4→ZnSO4+CuAssume that all the copper formed stays on the strip.
Relative atomic mass (ArA_rAr): Cu = 63.5 Zn = 65.4
What happens to the mass of the strip?
It increases, because copper is deposited on the strip.
It decreases, because each zinc atom that dissolves is replaced by one copper atom, which has a smaller mass.
It stays the same, because atoms are not created or destroyed in a reaction.
It increases, because zinc sulfate forms on the strip.
60 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.