For the following metal and non-metal combination reaction you have 3 moles of na. how many moles of cl2 would you need to add to have stoichiometrically equivalent amounts of na and cl2?

2na(s) + cl2(g) --> 2nacl(s)

The molar ratio of Na : Cl₂ is 2:1
Moles of Na present = 3
2/1 = 3/x
x = 1.5
1.5 moles of Cl₂ needed to have stoichometrically equivalent amount

The nucleus inside an atom consists of positively-charged  protons  and neutrally-charged  neutrons. a  proton  is a subatomic particle with a positive electric charge. allprotons  are identical.

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.