Gthe reaction; 4 ag(s) + o2(g) > 2 ag2o(s), is exothermic. which statement about the reaction is correct? (a) it is spontaneous at all temperatures. (b) it is spontaneous only at low temperatures. (c) it is spontaneous only at high temperatures. (d) it is non-spontaneous at all temperatures

The correct answer is B. It is spontaneous only at low temperatures.

Explanation:

In thermodynamics, the Gibbs free energy is a thermodynamic potential that can be used to calculate the maximum of reversible work that may be performed by a thermodynamic system at a constant temperature and pressure.

The spontaneity of a reaction is given by the equation:

ΔG = ΔH - TΔS

where:

ΔH: enthalpy variation

T: absolute temperature

ΔS: entropy variation

As the reaction is exothermic, ΔH<0

As the reaction order increases (the reagents are solid and gas and their product is solid), ΔS<0

Therefore, the reaction will be spontaneous when ΔG is negative.

ΔG = ΔH - TΔS

That is, the entropy term must be smaller than the enthalpy term.

Hence, the reaction will be spontaneous only at low temperatures.

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it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2