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Under standard conditions, the combustion of gas is most likely spontaneous since you would usually be releasing heat (-delta H) and increasing entropy (+delta S). However, I wouldn't say that combustion is always spontaneous, especially depending on non-standard conditions. For example, if you have a very high Q value (many products vs. little reactants), the delta G may be positive (not spontaneous).
I think most combustion reactions are spontaneous because they are exothermic, releasing heat, and usually cause an increase in gaseous substances, which have a higher value for entropy. It really depends on other determining factors, however.
In the case of ∆G° = ∆H° - T∆S°, which indicates standard condition yes. The combustion of gas will be spontaneous due to the negative enthalpy value, the release of heat through an exothermic reaction, and a positive (increasing) entropy.
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