In the electrochemical cell using the redox reaction below, the oxidation half-reaction is sn4+ (aq) + fe (s) → sn2+ (aq) + fe2+ (aq)

Fe(s)   ⇒ Fe²⁺  + 2e⁻ Oxidation

Explanation:

Oxidation is the loss of electrons, so what we have to do here is to determine the change in oxidation of the atoms in the reaction and identify the species which loses electrons.

Sn⁴⁺ + 2e⁻  ⇒  Sn²⁺   Reduction

Fe(s)   ⇒ Fe²⁺  + 2e⁻ Oxidation

Then the oxidation half-reaction is:

Fe(s)   ⇒ Fe²⁺  + 2e⁻ Oxidation

b. acid is the correct answer @jayxboof all social media

acid : acids are those which accepts an electron-pairs.

base : bases are those which donates ab electron-pairs.

alkali : it is a base that dissolves in water. it is basically a base and the ph greater than 7.

hydroxide ion : it is a poly-atomic ion which is negatively charged.

the dependant variable is spilled water

the independent is the heat