Question

What will occur if a block of copper metal is dropped into a beaker containing a solution of $ZnS{{O}_{4}}$?
A. The copper metal will dissolve with evolution of oxygen gas
B. No reaction will occur
C. The copper metal will dissolve with evolution of hydrogen gas
D. The copper metal will dissolve with zinc metal will be deposited

Answer 1

The standard reduction potential for $C{{u}^{2+}}|Cu$ is greater than that for $Z{{n}^{2+}}|Zn$.
Hence, $Zn$ is a better reducing agent than $Cu$ . Hence, $Zn$ can replace $Cu$ from copper sulphate solution.

Complete step by step solution:
At the point when the reactivity arrangement table is inspected, it is apparent that copper is less receptive than zinc.
At the point when a block of copper is put in Zinc sulfate arrangement, no reaction happens.
This since copper which is less reactive than zinc, doesn't dislodge zinc from zinc sulfate.
On the off chance that zinc is set in a copper sulfate arrangement, zinc being more responsive than copper goes through dislodging response and uproots copper from copper sulfate and structures a zinc sulfate arrangement.
Copper cannot displace zinc from $ZnS{{O}_{4}}$.

**The correct option is B. No reaction will occur.

Additional Information: **
Since Zinc is set much above Copper in the reactivity arrangement , so zinc is considerably more receptive than copper . In a galvanic cell , zinc is made the cathode since it can undoubtedly lose electrons and copper is made the anode since it can pick up electrons much effectively when contrasted with zinc because of its low reactivity.

Note:
In contrast, in the event that we submerge a copper strip in a zinc sulfate arrangement, no response will happen on the grounds that the opposite response is profoundly nonspontaneous, with a $+50.1\,kcal\,per\,mol$ free energy boundary to overcome.