There are several equations given below. Which equation can be used to find the standard entropy changes (ΔSo)happen in a reaction?     a. S° = (moles product × S°reactant) − (moles reactant × S°product)   b. S° = (moles product) × S°product − (moles reactant) × S°reactant   c. S° = (moles product × S°product) + (moles reactant × S°reactant)   d. S° = (moles reactant × S°reactant) − (moles product × S°product)   e. S° = (moles product × S°product) − (moles reactant × S°reactant)

A reaction has a positive entropy change. What would the sign of AHrxn need to be to make the spontaneity of the reaction temperature dependant? In this case, would the temperature have to decrease or increase to make it nonspontaneous? AHrxn > 0, temperature would have to increase to make the reaction nonspontaneous. AHTXN > 0, temperature would have to decrease to make the reaction nonspontaneous. Remove 5 points from my score, please. AHTXN < 0, temperature would have to decrease to make the reaction nonspontaneous.

Consider the reaction: 2H₂O (1) --> 2H₂(g) + O₂(g) Decrease in entropy (delta S 0)

For the following reactions, indicate whether the entropy of the system increases, decreases, or remains nearly the same. a. Al3+(aq) + 3 OH-(aq) → Al(OH)3(s)b. CaCO3(s) → CaO(s) + CO2(g)c. Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s)