Question

Assertion: Copper sulphate can be stored in a zinc vessel.
Reason: Zinc is less reactive than copper.

Answer 1

Analysing the assertion and reason:

The half -cell reactions are:
$C{u}^{2+}+2e^{-}\to Cu\left(s\right);E^{\circ }=0.34V$
$Z{n}^{2+}+2e^{-}\to Zn\left(s\right);E^{\circ }=0.76V$

The overall reaction is:
$C{u}^{2+}+Zn\left(S\right)\to Cu\left(S\right)+Z{n}^{2+}$
$E_{cell}^{\circ }=E_{cathode}^{\circ }{E}_{anode}^{\circ }$
$E^{\circ }=0.34V-(-0.76V)=+1.1V$

We know that $G^{\circ }=-nF{E}^{\circ }.$

Here, $E^{\circ }$ is postive. So, the value of $G^{\circ }$ will be negative , which means that the reaction is feasible.

Copper $\left(C{u}^{2+}\right)$ sulphate can not be stored in zinc vessels as zinc is more reactive than copper. Zinc is a stronger reducing agent than copper. Thus, zinc donates electrons to $\left(C{u}^{2+}\right)$, and the above redox reaction occurs.

Hence, both the assertion and the reason are false.

So, option (D) is the correct answer.