Predicting Spontaneity of 2CO(g)+O2(g)=2CO2(g)

[reconrusty]

Homework Statement

Will the following processes be spontaneous only at high temperatures, only at only temperatures, at all temperatures, or at no temperatures?

2CO(g)+O2(g)=2CO2(g)
Delta(H)=-566kJ

Homework Equations

The Attempt at a Solution

So i just need to figure out how to predict the sign of Delta(S) but I am not sure how to do that with just the balanced equation given, any tips would be helpful.

Thanks!

 

[Chestermiller]

I think this question is referring to the effect of temperature on the equilibrium constant. For an exothermic reaction (negative delta H), does the equilibrium constant increase with temperature or decrease with temperature?

Chet

 

[brake4country]

The total moles in the reactants are more than the products. This is decreasing entropy. If the total moles were more in the products, then this would be increasing entropy. So, when ΔH is negative, and ΔS<0 (decreasing entropy), we know that this is spontaneous at low temps.

The trends are as follows:
ΔS>0 and ΔH<0 Spontaneous (ΔG<0)
ΔS>0 and ΔH>0 spontaneous at high temps.
ΔS<0 and ΔH<0 spontaneous at low temps
ΔS<0 and ΔH>0 non-spontaneous (ΔG>0)

Notice that when the signs for both ΔS and ΔH are the same, it dictates the conditions of the reaction (H and S <0 are both spont. at low temps) and (H and S>0 are spont. at high temps). Hope this helps.