Question

In cyanide method, silver metal is obtained as given in the following reaction:
$2K\left[Ag{\left(CN\right)}_2\right]+Zn⟶K_2\left[Zn{\left(CN\right)}_4\right]+2Ag$
In this :

• A. $Ag$ has been oxidised and $Zn$ has been reduced
• B. $A{g}^{+}$ has been reduced and $Zn$ has been oxidised
• C. both the metals have been oxidised
• D. both the metals have been reduced

Answer 1

Answer: (B)

$A{g}^{+}$ has been reduced and $Zn$ has been oxidised

$2K\left[Ag{\left(CN\right)}_2\right]+Zn⟶K_2\left[Zn{\left(CN\right)}_4\right]+2Ag$
+1 0 +2 0
So here,
$A{g}^{+}$ reduces to $Ag$ and $Zn$ oxidises to $Z{n}^{+2}$.