disproportionation
ethanol can be oxidised to ethanal and further oxidised to ethanoic acid
The way to tackle this to look at reactants and at the products, and this where oxidation numbers come in. Remembering that oxidation is loss of electrons and reduction is gain, (OILRIG is an acronym that is sometimes used). Mn metal is changed to Mn2+ so it is oxidised H in HCl has a +1 oxidation number and in H2 zero so it is reduced. Cl in HCL is at -1 and is -1 in MnCl2 so it is neither oxidised nor reduced.
With 'sodium thiosulfate' (two words!) and bromine the reaction will be strong to give oxidised tetrathionate and reduced bromide: 2 S2O32−(aq) + Br2(aq) → S4O62−(aq) + 2 Br−(aq)
The reactant that reduces another atom
Mn(7+) is reduced to Mn(2+) going from purple to colourless/pale pink. The Fe(2+) ions are oxidised to Fe(3+) ions to complete the redox reaction.
No it is not. However, it is easily oxidised.
in the reaction of H2 and Cl2 hydrogen is oxidised. Chlorine is reduced.
Yes, rusting is oxidation of iron. The iron is oxidised, the oxygen is reduced. This is thus basically a redox reaction.
yes as zinc is oxidised and hydrogen is reduced
The arsenic iii ion is oxidised to arsenic V ion and iodine is reduced to iodide.
It reacts with it. The reaction is a redx reaction. Nitrogen is reduced (its oxidation number goes from 0 to -3) and hydrogen is oxidised (its oxidation number goes from 0 to +1)
Silver cations are reduced.
ethanol can be oxidised to ethanal and further oxidised to ethanoic acid
Zero- red phosphorus is an allotrope of phosphorus, a form of the element. By definition elemnts are considered to be neither oxidised or reduced.
You cannot 'burn' MgO, it is refactory. I take it you mean burning Magnesium metal in oxygen - if so the answer is that the magnesium is oxidised to MgO and the oxygen is reduced - all reduction/oxidation ('redox') reactions are coupled - if something is oxidised the other is reduced.
An element is REDUCED. By that, it means that an element of a compound or an element in itself has gained electron/s when the reaction occurs. You can find this out when you see a change in their oxidation number.
Chromium