(a(i))[2]
Balance the equation and show state symbols: $\text{CuSO}_4(\,) + \text{KI}(\,) \rightarrow \text{CuI}(\,) + \text{I}_2(\,) + \text{K}_2\text{SO}_4(\,)$
(a(ii))[1]
Deduce the oxidation number of copper in $\text{CuSO}_4$ and $\text{CuI}$.
(a(iii))[2]
Describe the type of reaction shown by the equation in part (a)(i). Explain your answer in terms of electron transfer.
(b)[4]
In the reaction described in part (a)(i), a student uses $17.43\,\text{g}$ of $\text{CuSO}_4\cdot y\text{H}_2\text{O}$. After further titration of the reaction products, the student finds that the total amount of $\text{CuSO}_4$ in the sample is $0.0982\,\text{mol}$. Use the Data Booklet to complete the table and calculate the value of $y$, where $y$ is an integer. Show your working.