Reaction of zinc with copper sulphate solution is: 

When zinc is added to copper sulphate solution, it displaces copper from the solution and forms a zinc sulphate solution. Because zinc is more reactive than copper in the reactivity series, it will undergo a redox reaction known as the displacement reaction of metal.
 

But, first and foremost, it is dependent on the oxidation state of the copper, as copper is a transition metal with varying oxidation states. There is copper (I), copper (II), and even copper (III) (III). In order for the reaction to occur, the copper sulphate must be in an aqueous state, dissolved in water.
The full chemical equation would be as follows:
$\mathrm{Zn}(\mathrm{s})+{\mathrm{CuSO}}_4(\mathrm{aq})\to {\mathrm{ZnSO}}_4(\mathrm{aq})+\mathrm{Cu}(\mathrm{s})$

The copper deposit will be reddish brown, and the copper (II) sulphate solution will be a less blue (paler) $\text{CuSO}4$ solution is blue, whereas the ${\text{ZnSO}}_4$ solution is colourless.

The Ionic Equation is as follows:$\text{Zn}\left(\text{s}\right)+{\text{Cu}}^{2+}\left(\text{aq}\right)\to {\text{Zn}}^{2+}\left(\text{aq}\right)+\text{Cu} \left(\text{s}\right)$

Hence, the correct option is (C).