Question

A galvanic cell consists of a strip of cobalt metal dipping into 1.0 M $C{o}^{2+}$ ions, and another half cell in which a piece of platinum dips into a 1.0 M solution of $C{l}^{-}$ ions. Now $C{l}_2\left(g\right)$ at a pressure of 1.0 atm is passed into this solution. The observed cell voltage is 1.63 V, and as the cell reaction proceeds, the Co electrode becomes negative.
$E^{\ominus }(1/2C{l}_2+e^{-}\to C{l}^{\ominus })=1.36V$

Assertion: The cell voltage increases, if pressure of $C{l}_2\left(g\right)$ is increased.

Reason: Difference in cell voltage is directly proportional to the pressure of $C{l}_2\left(g\right)$.

• A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion
• B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
• C. Assertion is true but Reason is false
• D. Assertion is false but Reason is true
• E. Both Assertion and Reason are false
  

Answer 1

The correct option is C Assertion is true but Reason is false

$E_{cell}=E_{cell}^{\ominus }-\frac{0.059}{2}log\frac{\left[C{I}^{\ominus }{]}^2\right[C{o}^{2+}]}{P_{C{l}_2}}$
If pressure of $C{l}_2$ is increased, then cell voltage will increase.