Question

1 of 1 1) Balance the following redox reaction: Al + Zn → A1 + Zn 2. Balance the follwoing unbalanced chemical equations. Then, write an ionic equation, and a net ionic equation for each equation. Identify the spectator ions a) CaCl(aq) + K3PO(aq) - KClaq) + CaPO(S) LiOH(aq) + H2SO4(aq) → H01) + LigSO4(s) 3. In the reactions a) Pb(s) + 2Ag (aq) - P** (aq) + 2Ag(s) b) FeO3(s) + 3C0(g) 3Fe(s) + 3C0 g) Which species are oxidized and which are reduced? Which species are the oxidizing agents and which are the reducing agents? 4) Identify as oxidation or reduction. Give the reason of your choice. a) Zn2+ 2e - Zn b) Pb - Pb2+ 2e c) Cl2 + 2e-201 d) Al-A! + 3e

Answer 1

1. The required balanced redox reaction is

2 Al + 3 Zn⁺² $\rightarrow$ 2 Al⁺³ + 3 Zn

To balance a given reaction, we need to balance the number of different atoms on right side to the number of different atoms on left side.

The charge on both sides of the arrow should also be balanced

In the given balanced equation, there are 2 Aluminium atoms on left and 2 Aluminium ions on right side

There are three Zn ions on left side and three Zinc atoms on right side

The number of Al atoms on right side is equal to the number of Al atoms on left side

The number of Zn atoms on right side is equal to the number of Zn atoms on left side

The charge is also balanced on both sides.

To balance the given unbalanced reaction it is better to start balancing from the charge.

Zinc is in +2 oxidation state and Aluminium is in +3 oxidation state. We need to equal the charge on both sides. For this 3 Zinc atoms are taken to make the charge on left side +6 and 2 Aluminium atoms are taken on right side to make the charge on right side +6.

Then the neutral atoms are balanced accordingly.