The redox reaction $Z n (s) + P b {C l}_{2} (a q) ⟶ P b (s) + Z n {C l}_{2} (a q)$ can be represented as following half equations : $Z n (s) ⟶ {Z n}^{2 +} (a q) + 2 e^{-}$ (oxidation) and ${P b}^{2 +} (a q) + 2 e^{-} ⟶ P b (s)$ (reduction).
If true enter 1, else enter 0.
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Solution

The correct option is A 1
Redox reaction is $Z n (s) + P b {C l}_{2} (a q) ⟶ P b (s) + Z n {C l}_{2} (a q)$ .
The complete ionic equation is $Z n (s) + P b^{2 +} (a q) + 2 {C l}^{-} (a q) ⟶ P b (s) (a q) + Z n^{2 +} (a q) + 2 {C l}^{-} (a q)$ .
The net ionic equation is $Z n (s) (a q) + P b^{2 +} (a q) ⟶ P b (s) + Z n^{2 +} (a q)$ .
Thus, it can be represented as following half equations :
$Z n (s) ⟶ {Z n}^{2 +} (a q) + 2 e^{-}$ (oxidation)
and
${P b}^{2 +} (a q) + 2 e^{-} ⟶ P b (s)$ (reduction)

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