Based on the activity series, which one of the reactions below will occur? Based on the activity series, which one of the reactions below will occur? 3FeBr2 (aq) + 2Au (s) → 3Fe (s) + 2AuBr3 (aq) SnCl2 (aq) + Cu (s) → Sn (s) + CuCl2 (aq) Zn (s) + MnI2 (aq) → ZnI2 (aq) + Mn (s) 2AgNO3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq) 3Hg (l) + 2Cr(NO3)3 (aq) → 3Hg(NO3)2 + 2Cr (s)

Answer : The reaction takes place will be,

(d)

Explanation :

Single replacement reaction : A chemical reaction in which the more reactive element replace the less reactive element.

It is represented as,

In this reaction, A is more reactive element and B is less reactive element.

Reactivity series : It is used to determine the products of the single displacement reactions. As we know that in a single displacement reaction, the most reactive metal displaces the least reactive metal.

(a)

Gold (Au) metal is less reactive metal than Fe metal, So, it can not displaces Fe metal from its solution. Thus, this reaction will not takes place.

(b)

Copper (Cu) metal is less reactive metal than Sn metal, So, it can not displaces Sn metal from its solution. Thus, this reaction will not takes place.

(c)

Zinc (Zn) metal is less reactive metal than Mn metal, So, it can not displaces Mn metal from its solution. Thus, this reaction will not takes place.

(d)

Lead (Pb) metal is more reactive metal than Ag metal, So, it can displaces Ag metal from its solution. Thus, this reaction will takes place.

(e)

Mercury (Hg) metal is less reactive metal than Cr metal, So, it can not displaces Cr metal from its solution. Thus, this reaction will not takes place.

Hence, the reaction takes place will be,

(d)

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