In which of the following processes is iron being oxidized?

1 Fe + H₂SO₄ → FeSO₄ +H₂

2 FeSO₄ + H₂S → FeS + H₂SO₄

3 2FeCI₂ + Cl₂ → 2FeCl₃

4 2FeCl₃ + SnCl₂ + → 2FeCl₂ + SnCl₄

Emmyoguji

6 years ago

In reaction 1 the oxidation number of fe increases from 0 to +2 from left to right. In reaction 2, the oxidation state of fe remain constant for both sides and implies no reduction no oxidation. In reaction3 the oxidation state of fe increases from +2 to +3 from left to right .in reaction 4 the oxidation state of fe decrease from +3 to +2 from left to right . therefore, fe is oxidized in reaction 1and 3. Option D is correct

Kenhinde

3 years ago

No.1
Fe- FeSO4
X=0 - x+(+6)+4(-2)
X+6-8=0
X=0+8-6
X=+2
So...it moves from 0 to +2🙂 Gracia's

Peterpaul090

6 years ago

Please wat is the right answer

Kenhinde

3 years ago

No.2 to be continued 😄🚵🚵🚵😄

Kenhinde

3 years ago

FeCl2 - FeCl3
X+2(-1) - X+3(-1)
X-2=0 - X-3=0
X=0+2 - X=0+3
X=+2 - X=+3
So...it increases from +2 to +3 0xidation(Oxidized), reducing agent

Vkook

7 years ago

wrong answer

ebunerise

2 years ago

oxidation involves the loss of electrons so no 1 cannot be correct since the oxidation number increased from 0 to +2 ..

Oxidation is the loss of electrons during reaction by a molecule, atom or ion. In terms of electron transfer, oxidation is defined as the phenomenon in which an atom loses electron to form a positively charged cation. During formation of ionic bond one atom undergoes oxidation while another atom undergoes reduction.