The following reaction is found to be endothermic (δh > 0), the entropy change is negative, and therefore the gibbs free energy is positive at all temperatures. does this mean that this reaction could never be spontaneous? for the reaction below at 25 °c, δgºrxn = 326.4 kj. calculate the partial pressure of ozone, o3(g), needed to make this reaction spontaneous if the partial pressure of oxygen is 0.21 atm.

as we know our atmosphere or air have different levels. every level has other gasses, and every gas has another permeability. when the light comes from lower permeability to higher permeability, it changes its direction. so that means that when the light comes from the moon to the earth, it changes it's direction many more times. it basically means that the shape of the light part of the moon is changed on the earth.

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