Which of the following options are correct for the reaction
$$2\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s}) \rightarrow 2 \mathrm{Au}(\mathrm{s})+\left[\mathrm{Zn}(\mathrm{CN})_{4}\right]^{2-}(\mathrm{aq})$$
A. Redox reaction
B. Displacement reaction
C. Decomposition reaction
D. Combination reaction
Choose the correct answer from the options given below:
Solution
$2\left[\stackrel{+1}{\mathrm{Au}}(\mathrm{CN})_2\right]^{-}+\stackrel{0}{\mathrm{Z}} \mathrm{n}(\mathrm{s}) \longrightarrow 2 \stackrel{0}{\mathrm{Au}}+\left[\stackrel{+2}{\mathrm{Zn}}(\mathrm{CN})_4\right]^{-2}$<br/><br/>$\mathrm{Zn}$ displaced $\mathrm{Au}^{+}$<br/><br/>
Reduction and Oxidation both are taking place.
About this question
Subject: Chemistry · Chapter: Redox Reactions · Topic: Oxidation States
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