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(A) The given reaction is $2[Au(CN)_2]_{(aq)}^{-} + Zn_{(s)} \rightarrow 2Au_{(s)} + [Zn(CN)_4]_{(aq)}^{2-}$.Assigning oxidation states: $2[\stackrel{

Vedclass · Accepted Answer

$A$ and $B$ only

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(A) The given reaction is $2[Au(CN)_2]_{(aq)}^{-} + Zn_{(s)} \rightarrow 2Au_{(s)} + [Zn(CN)_4]_{(aq)}^{2-}$.Assigning oxidation states: $2[\stackrel{+1}{Au}(CN)_2]_{(aq)}^{-} + \stackrel{0}{Zn}_{(s)}$ $\rightarrow 2\stackrel{0}{Au}_{(s)} + [\stackrel{+2}{Zn}(CN)_4]_{(aq)}^{2-}$.Here,$Zn$ is oxidized from $0$ to $+2$ and $Au$ is reduced from $+1$ to $0$. Since both oxidation and reduction occur,it is a redox reaction.$Zn$ displaces $Au$ from the complex,making it a displacement reaction.Therefore,both $A$ and $B$ are correct.

Which of the following options are correct for the reaction
$2[Au(CN)_2]_{(aq)}^{-} + Zn_{(s)} \rightarrow 2Au_{(s)} + [Zn(CN)_4]_{(aq)}^{2-}$
$A.$ Redox reaction
$B.$ Displacement reaction
$C.$ Decomposition reaction
$D.$ Combination reaction
Choose the correct answer from the options given below:

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Which of the following options are correct for the reaction$2[Au(CN)_2]_{(aq)}^{-} + Zn_{(s)} \rightarrow 2Au_{(s)} + [Zn(CN)_4]_{(aq)}^{2-}$$A.$ Redox reaction$B.$ Displacement reaction$C.$ Decomposition reaction$D.$ Combination reactionChoose the correct answer from the options given below: