Spontaneous reactions?

Question

2 reactions:
a) H2O (s)-->H2O(l) delta H(enthalpy)=6.0 kJ, delta S (entropy)=22.1 J/K*mol
b) CaCO3(s)-->CaO(s)+CO2(g) delta H= 178kJ

which of the following is correct?
I. the reactions are spontaneous and exothermic.
II. both reactions occur with an increase in the system's disorder
III. the entropy change (deltaS*) for equation a is most likely positive.

its either I only, I and II only, II and III only, none, or all of the statements.

im confused. Because i cant tell when a reaction is spontaneous? i know that the entropy for a is 22.1 J/K (it wasnt given in the question, i figured it out to be that).
any help please??!
thanks!!!!

Answer 1

A reaction tends to be spontaneous if it causes an increase in the entropy of the system, and/or a decrease in the enthalpy of the system

Both reactions are endothermic (increase in enthalpy) becuase of positive delta H values.
Both have an increase in entropy (positive delta S value for the first one, production of a gas for the second)

So I'd say statements ll and lll are true.

Answer 2

that's actual...The correct equation is: DG = DH - TDS to make certain that the reaction to be spontaneous, DeltaG must be under 0. If Delta S is detrimental, the -TDS term would be advantageous. as long as DeltaH is greater detrimental than TDS is advantageous, the reaction would be spontaneous. An occasion of this occasion is the freezing of water at temperatures under 0C. The entropy of the water decreases regardless of the shown fact that it is likewise exothermic (DeltaH < 0). desire that facilitates...