1) write the formula of the conjugate acid: HCO2-

2) write the formula of the conjugate base:
C6H5NH2

3) write the formula of the conjugate acid of the brønsted-lowry base:
HCO3-

4) write the formula of the conjugate acid of the brønsted-lowry base:
C6H5NH2

5) write the acidic equilibrium equation for HC2H3O2

6) write the basic equilibrium equation for C6H5NH2

7) write the basic equilibrium equation for NH3

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.

The answer you are looking for is option d

Product should she record in last row of the table

rosa was looking for patterns to predict the products of chemical reactions. she recorded three similar decomposition reactions in the table.she should record 2licl + 3o2.

in the last row of the table. it is the thermal decomposition of chlorate lithium, hence, she should record these products as: lithium chloride ( 2licl ) and oxygen ( 3o2 )   2 > 2 licl + 3o2.