Predict whether each of the following reactions would be spontaneous or non spontaneous under standard conditions or if it is impossible to tell with the data given.

a)2KClO3(s)+3C(s)-->3CO2(g)+2KCl(s) Exothermic

b) 2NO(g) + O2(g) ---> 2NO2(g) Exothermic

c)H2(g)+Zn(ClO3)2(s)-->2HClO3(l)+Zn(s) Endothermic

Does information come from the state the elements are in from reactant to product? I know that the exo/endothermic is useful but I do not remember how to use it.

Frankly, I think there is insufficient information for all of them. You need delta G. In a general sense exothermic reactions (delta H is -) often are spontaneous unless delta S screws things up and endothermic reactions (delta H is +) unless delta S screws things up. Technically, however, you need both delta H as well as T and delta S so you can calculate delta G from dG = dH - TdS.

In the problem it states if the reactions underwent standard conditions, would that mean they would all have the same temperature and delta s meaning the only thing that would ,make the difference is the delta H?

I think standard conditions in this case means 25 C and 1 atm and ALL will have those conditions. What counts is dH and dS where

dHrxn = (n*dHf products) = (n*dHf reactants) and
dSrxn = (n*dSf products) - (n*dSf reatants) or
dGrxn = (n*dGf products) - (n*dGf reactants)

To predict whether a reaction is spontaneous or non-spontaneous under standard conditions, you can use two factors: the change in enthalpy (∆H) and the change in entropy (∆S). These factors help determine the Gibbs free energy change (∆G) for the reaction.

The Gibbs free energy change is given by the equation ∆G = ∆H - T∆S, where T is the temperature in Kelvin.

If ∆G is negative, the reaction is spontaneous in the forward direction under standard conditions. If ∆G is positive, the reaction is non-spontaneous under standard conditions. If ∆G is zero, the reaction is at equilibrium.

Now, let's analyze each reaction:

a) 2KClO3(s) + 3C(s) → 3CO2(g) + 2KCl(s) (Exothermic)

To determine the spontaneity, we need the enthalpy change (∆H) and the entropy change (∆S). Unfortunately, you didn't provide this information. However, we can make a general prediction based on the given information that the reaction is exothermic.

Generally, exothermic reactions tend to be spontaneous because they release energy. So, based on this information, we can predict that this reaction is likely to be spontaneous under standard conditions.

b) 2NO(g) + O2(g) → 2NO2(g) (Exothermic)

Again, we lack the specific ∆H and ∆S values. However, we know that the reaction is exothermic, which implies that ∆H is negative. Exothermic reactions often favor spontaneous reactions.

In this case, the reaction involves the formation of more moles of gas compared to the reactants, which results in an increase in entropy (∆S > 0). When ∆H is negative and ∆S is positive, it is more likely that the reaction is spontaneous under standard conditions.

c) H2(g) + Zn(ClO3)2(s) → 2HClO3(l) + Zn(s) (Endothermic)

Once again, specific ∆H and ∆S values are not provided. However, we know that the reaction is endothermic, suggesting that ∆H is positive. Endothermic reactions absorb energy from the surroundings.

In this case, the reaction involves a decrease in the number of gas moles, which results in a decrease in entropy (∆S < 0). When ∆H is positive and ∆S is negative, the reaction is less likely to be spontaneous under standard conditions.

Keep in mind that without the specific values of ∆H and ∆S, we can only make general predictions based on the given information. For more accurate predictions, you would require the specific values to calculate ∆G.