The ferrous oxide is the oxdant.
O2
The ion MnO4 is reduced toMnO2 and sulfur is oxidized to ion sulfate. Sulfite is the reducing agent.
Bromine is the oxidizing element.
As a rule of thumb, if elemental hydrogen is in a reaction and it's NOT reacting with a metal, it's the reducing agent.
Cu is oxidized. The oxidation number goes from 0 in Cu to +2 in CuSO4. S is reduced. The oxidation number goes from +6 in H2SO4 to +4 in SO2. The oxidizing agent is H2SO4 since it causes Cu to be oxidized. The reducing agent is Cu since it causes S in H2SO4 to be reduced.
O2
Zn alone is a reducing agent because it donates electrons during a reaction and H2SO4 alone is an oxidizing agent because it may donates atomic oxygen during the reaction but (Zn + H2SO4) mixture is a reducing agent because this mixture may produce atomic hydrogen during a reaction.
Neutralization reaction.2HCl + Ca(OH)2 ==> CaCl2 + 2H2OThis is NOT an oxidation-reduction reaction.
CuCl2
The ion MnO4 is reduced toMnO2 and sulfur is oxidized to ion sulfate. Sulfite is the reducing agent.
Bromine is the oxidizing element.
H3o+
It is safer to claim it as neither - not least because the reaction would/does not work. Far safer to say that the sulphur is oxidised (which, you could argue, makes it a reducing agent).
This is a net ionic equation from a double replacement reaction. There should have been 2H+, otherwise the equation doesn't balance. 2H+ + 2CrO42- --> Cr2O72- + H2O
It is a combustion reaction, which is a reaction in which a substance combines with oxygen, releasing a large amount of energy in the form of light and heat.
Tin and iron are being oxidized because to be oxidized is to lose electrons. Chlorine is being reduced, because it gains electrons.
The reaction of an acid plus a base will result in the formation of a salt plus water.