Consider the following reaction. 2 Fe2O3(s) + 3 C(s) = 4 Fe(s) + 3 CO2(g) AH° = +467.9 kJ and AS° = +558.4J/K
Which of the following statements is correct?
The reaction is neither enthalpy-driven nor entropy-driven.
The reaction is not enthalpy-driven, but it is entropy-driven.
The reaction is enthalpy-driven, but it is not entropy-driven.
The reaction is enthalpy-driven and entropy-driven.

Consider the same reaction in the first question.
Determine the temperature above or below which the reaction becomes spontaneous under the standard conditions.
Below 275 K
Below 838 K
Above 275 K
Above 838 K
Below 542 K
Above 542 K

Nonmetals usually react by gaining electrons

Ijust took the quiz. their is no coefficient needed. : )

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.