Balance the oxidation adn reduction half-reactions for the iron (ii) ion and permanganate ion 2.. how many moles of fe2+ ions can be oxidized by .067 moles of mno4-ions

Fe²⁺ ion gets oxidised to Fe³⁺ ion and permanganate ion (MnO₄⁻) gets reduced to Mn²⁺ ion.  Fe²⁺ ion acts as reducing agent and MnO₄⁻ ion acts as oxidising agent. The half cell reactions are as follows:

5Fe²⁺ → 5Fe³⁺  +  5e    (reaction at anode)

MnO₄⁻ + 8H⁺ + 5e → Mn²⁺ + 4 H₂O   (reaction at cathode)

The overall reaction is MnO₄⁻ + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ 4 H₂O.

As per balanced redox reaction 1 mole MnO₄⁻ can oxidise 5 moles of Fe²⁺ ion. So, 0.067 moles of MnO₄⁻ can oxidise 5 X 0.067= 0.335 moles of Fe²⁺ ion.

its first and third is your answer i did the qustion the fourth isnt right

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.