Identify the atoms that are oxidized and reduced, the change in the oxidation state for each, and oxidising and reducing agents in each of the following equations:
(a)mg + nicl2 -> mgcl2 + ni
(b)pcl3 + cl2 -> pcl5
(c)c2h4 + 3o2 -> 2co2 + 2h2o
(d)zn + h2so4 -> h2 + znso4
(e)2k2s2o3 + i2- > k2s4o6+2ki
(f)3cu + 8hno3 = 3cu(no3)2 + 4h2o + 2no

Explanation:

a)

Oxidation state of Mg changes to 0 to +2.

Oxidation state of Ni changes to +2 to 0.

Oxidation state of Cl does not change.

So, Mg is oxidized, Ni is reduced.

Mg acts as reducing agent and acts as oxidizing agent.

b)

Oxidation state of P changes to +3 to +5.

Oxidation state of Cl changes to 0 to -1.

So,

P is oxidized and Cl is reduced.

acts as reducing agent and acts as oxidizing agent.

c)

Oxidation state of C changes to -2 to +4.

Oxidation state of O changes to 0 to -2.

Oxidation state of H does not change.

So,

C is oxidized and O is reduced.

acts as reducing agent and acts as oxidizing agent.

d)

Oxidation state of Zn changes to 0 to +2.

Oxidation state of H changes to +1 to 0.

Oxidation state of S and O do not change.

So, Zn is oxidized, H is reduced.

Zn acts as reducing agent and acts as oxidizing agent

e)

Oxidation state of S changes to +2 to +2.5.

Oxidation state of I changes to 0 to -1.

Oxidation state of K and O do not change.

So, S is oxidized, I is reduced.

acts as reducing agent and acts as oxidizing agent.

f)

Oxidation state of Cu changes to 0 to +2.

Oxidation state of N changes to N +5 to +2.

Oxidation state of H and O do not change.

So, Cu is oxidized, N is reduced.

Cu acts as reducing agent and acts as oxidizing agent

step-by-step explanation:

whole numbers, zero or greater

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