Question

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 1

Answer : The reaction takes place will be,

(d) $2AgNO_3(aq)+Pb(s)\rightarrow 2Ag(s)+Pb(NO_3)_2(aq)$

Explanation :

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

It is represented as,

$A+BC\rightarrow AC+B$

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) $3FeBr_2(aq)+2Au(s)\rightarrow 3Fe(s)+2AuBr_3(aq)$

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) $SnCl_2(aq)+Cu(s)\rightarrow Sn(s)+CuCl_2(aq)$

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) $MnI_2(aq)+Zn(s)\rightarrow Mn(s)+ZnI_2(aq)$

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) $2AgNO_3(aq)+Pb(s)\rightarrow 2Ag(s)+Pb(NO_3)_2(aq)$

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) $2Cr(NO_3)_2(aq)+3Hg(l)\rightarrow 2Cr(s)+3Hg(NO_3)_2(aq)$

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) $2AgNO_3(aq)+Pb(s)\rightarrow 2Ag(s)+Pb(NO_3)_2(aq)$

Answer 2

Based on the activity series, the reaction that will occur is;  2AgNO3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq)

We must note that the activity series shows the order of reactivity of elements. The elements that are higher in the series displaces elements that are lower in the series from their aqueous solution.

If we look at all the reactions listed, we will discover that the reaction 2AgNO3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq) is possible because Pb is higher than Ag in the activity series hence Pb displaces Ag from its aqueous solution.

Learn more: https://brainly.com/question/12989252