Chemistry--Dynamic Equilibrium?

Question

Please help me figure out this homework question:

"At 800 degrees C, the equilibrium constant for the reaction CO2 + H2 <--> CO + H20 is .279. At a different temperature the equilibrium constant is 0.100. Is this different temperature higher or lower than 800 degrees? Give your reasoning."

Thank you!

Answer 1

The equilibrium constant rises as you have more products than reactants, so the temperature is lower (less energy is being put into the reaction).

Answer 2

on the distinctive temperature, the ok fee has decreased this shows which you have lots much less products and better reactants or that the reaction has shifted to the left if the reaction is exothermic, raising the temperature will shift the reaction to the left (heat temperature would desire to need to be seen as a product) and this shows the 2nd temperature is extra suitable than the 800 if the reaction is endothermic, reducing the temperature will shift the reaction to the left (heat temperature would desire to need to be seen as a reactant) and this shows that the 2nd temperature is shrink than the 800 you would be able to be sure if the reaction is endothermic or exothermic via technique of checking everyday enthalpy values on your textbook - utilising those values, this reaction would desire to be endothermic and reducing the temperature would desire to shift the reaction to the left because of the fact ok decreases - this shows that the 2nd temperature is shrink than 800 stages this appears like a bad question to me - you will desire to have been advised regardless of if the reaction grew to alter into endothermic or exothermic interior the venture