Question

Given $E_{A{g}^{\oplus }|Ag}^{\oplus }=0.80V$$E_{H^{\oplus }|H_2\left(Pt\right)}^{\oplus }=0.00V$ .

Assertion: $1.0M{H}^{\oplus }$ solution under $H_{2}S{O}_4$ at 1.0 bar $(\approx 1.0atm)$ is capable of oxidizing silver metal in the presence of 1.0 M $A{g}^{\oplus }$ ion.
Reason: $E_{cell}^{\oplus }$ is positive.

• 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 E Both Assertion and Reason are false

Anode : $Ag\to A{g}^{\oplus }\left(1M\right)+e^{-}$
$E^{\oplus }=0.80V$
Cathode : $2H^{\oplus }\left(1M\right)+2e^{-}\to H_2$
$E^{\oplus }=0V$
$E_{cell}^{\oplus }=-0.80<0$
$\Rightarrow$ Cell is not spontaneous.
So Ag metal cannot be oxidized.