A student made the following observations in the laboratory.

I. Clean copper metal did not react with $1$ molar $P b (N O_{3})_{2}$ solution
II. Clean lead metal dissolved in a $1$ molar $A g N O_{3}$ solution and crystals of $A g$ metal appeared
III. Clean silver metal did not react with $1$ metal $C u (N O_{3})_{2}$ solution

The order of decrease in reducing character of three metals is:

P b, C u, A g

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P b, A g, C u

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C u, A g, P b

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C u, P b, A g

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Solution

The correct option is A $P b, C u, A g$
The order of decrease in reducing character of three metals is $P b > C u > A g$ .

$P b$ has maximum reducing power. Hence, $P b$ can reduce both copper ions and silver ions.

$A g$ has a minimum reducing power. Hence, it can neither reduce copper ions nor reduce lead ions.

The reducing power of $C u$ is higher than that of $A g$ but lower than that of $P b$ . Hence, $C u$ can reduce silver ions but $C u$ cannot reduce lead ions.

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Similar questions

P b (N O_{3})_{2}

A g N O_{3}

C u (N O_{3})_{2}

P b + C u (N O_{3})_{2} \to P b (N O_{3})_{2} + C u

C u + A g (N O_{3})_{2} \to C u (N O_{3})_{2} + A g

Z n + P b (N O_{3})_{2} \to Z n (N O_{3})_{2} + P b

A g^{+}

C u^{2 +}

Given: $F e_{(s)} \to F e^{2 +} + 2 e^{-}; E^{o} = + 0.44 V$

$P b_{(s)} \to P b^{2 +} + 2 e^{-}; E^{o} = + 0.13 V$

$A g^{+} e^{-} \to A g; E^{o} = + 0.8 V$

$C u^{2 +} 2 e^{-} \to C u; E^{o} = + 0.34 V$

Which of the following metals will oxidise iron?

a) $A g$

b) $C u$

c) $P b$

d) None of these

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