00 Hydrogen peroxide decomposes to produce water
and oxygen. The equation is:
2H,02(g) → 2H2O(g) + O2(g)
Using the following values, calculate the heat change
for the reaction and say whether it is exothermic or
endothermic. Bond energies:
0-0 = 144 kJ/mol
0-H = 464 kJ/mol
O=0 = 498 kJ/mol

Ametal with a large number of free flowing electrons most likely has good conductivity

The answer to this is the 3rd choice!

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.