Effect of Temperature on GIbbs Free Energy

Imagine a reaction in which you decompose liquid water to produce oxygen gas and hydrogen gas:

H₂O_(l) → H_2(g) + ½O_2(g)

The reaction is endothermic, ΔH > 0, and the change in entropy is also positive, ΔS > 0
At room temperature and pressure this reaction is not spontaneous ( ΔG > 0).
But could I heat, or cool, the reaction sufficiently to make the reaction spontaneous?
Can I turn a nonspontaneous reaction into a spontaneous reaction by changing the temperature?
Want to know?
Go to https://www.ausetute.com.au/gibbstemp.html

AUS-e-TUTE Members can access the tutorial, game, test and exam by logging-in to the Members Only area of the website.

Gibbs Free Energy and Spontaneity of Reactions

Whether or not a chemical reaction proceeds in a particular direction depends on a balance between the enthalpy of the system and its entropy.
Gibbs Free Energy allows us to quantify this relationship, and determine whether a particular reaction will be spontaneous.
AUS-e-TUTE members can now access a new tutorial, game, test and exam on this topic.
Not a member?
There is a "free-to-view" tutorial currently available at http://www.ausetute.com.au/freeenergy.html

Spontaneous Chemical Reactions

What makes a chemical reaction spontaneous?
If I add hydrochloric acid (HCl_(aq)) to metallic magnesium (Mg_(s)), bubbles of hydrogen gas (H_2(g)) are given off and the remaining solution contains chloride ions and magnesium ions (MgCl_2(aq)):

Mg_(s) + 2HCl_(aq) → H_2(g) + MgCl_2(aq)

But if I try to bubble hydrogen gas through an aqueous solution of magnesium chloride, nothing happens. No solid magnesium forms! Why?
AUS-e-TUTE has just added a new tutorial, game, test and exam to help you understand what makes a reaction spontaneous, nonspontaneous, reversible or irreversible.
AUS-e-TUTE Members should log-in to use these new resources (listed under Thermodynamics in the Physical Chemistry section).

Not an AUS-e-TUTE Member?
A "free-to-view" spontaneous reactions tutorial is currently available for evaluation purposes at:
http://www.ausetute.com.au/spontaneous.html