The equilibrium constant of the reaction at 27 ∘ C and at 127 ∘ C are 1 . 6 × 10 - 3 and 7 . 6 × 10 - 2 respectively. Is the reaction exothermic or endothermic.

As the value of equilibrium constant increases with increase in temperature so, the reaction is endothermic in nature. If equilibrium constant increases with an increase in temperature, the reaction shifts to the right. The position of equilibrium also changes if you change the temperature. According to Le-Chatelier's Principle, the position of equilibrium moves in such a way as to tend to undo the change that you have made. If you increase the temperature, the position of equilibrium will move in such a way as to reduce the temperature again. It will do that by favouring the reaction which absorbs heat

What kind of equilibrium constant can be calculated from ∆ G ∘ value for a reaction involving only gases?

For reaction involving gases only. ∆ G ∘ = - 2 . 303 RT log K p ∴ K p can be calculated if ∆ G ∘ is known. Where, ∆ G ∘ = Change in standard Gibbs free energy. R = 0 . 0820575 atm mol - 1 K - 1 or 8 . 31447 J mol - 1 K - 1 T = Temperature in kelvin K p = Equilibrium constant with respect to pressure