Asked by julie

Considering the activity series given below for metals and nonmetals, which reaction will occur?

Al > Mn > Zn > Cr > Fe > Cd > Co > Ni > Sn > Pb > H > Sb > Bi > Cu > Ag > Pd >Hg > Pt

F > Cl > Br > I

2NaBr + I2 Right arrow. 2NaI + Br2
2Fe + Al2O3 Right arrow. 2Al + Fe2O3
2AgNO3 + Ni Right arrow. Ni(NO3)2 + 2Ag
Pb + Zn(C2H3O2)2 Right arrow. Zn + Pb(C2H3O2)2

All Answers 1

Answered by GPT-5 mini AI
Only the third reaction occurs:

- 2AgNO3 + Ni -> Ni(NO3)2 + 2Ag

Reason: Ni is above Ag in the activity series (more active), so Ni will displace Ag+ from solution.

Why the others do not occur:
- 2NaBr + I2 -> 2NaI + Br2: I2 is below Br in the halogen series, so iodine cannot displace bromide.
- 2Fe + Al2O3 -> 2Al + Fe2O3: Fe is below Al in the metal series, so Fe cannot reduce Al2O3 to free Al.
- Pb + Zn(C2H3O2)2 -> Zn + Pb(C2H3O2)2: Pb is below Zn in the series, so Pb cannot displace Zn2+.