Is the reaction Exothermic or Endothermic?

Question

Equilibrium constants and temperature follow this pattern:

300 Celsius - 4.34 x 10^-3

500 Celsius - 1.45 x 10^-5

600 Celsius - 2.25 x 10^-6

Can someone explain what this means in the following terms:

1) Is the reaction exothermic or endothermic?

2) Is the Delta H positive or negative?

3) Is the "heat" in the reaction a product or a reactant?

Appreciation is guaranteed to those who answer fully ^^

Answer 1

based on the info you gave I am not sure.

It depends on the delta H. If the Delta H is negative it is exothermic, if it is positive than it is Endothermic.

To find out what the delta H is you can use delta S and delta G.

use the following:

Delta G = Delta H+ T X Delta S

[T-----the temperature in kelvin which is Celsius + 273]

note: If delta G is positive than delta S is negative and the other way around.

Answer 2

One factor that affects equilibrium is temperature.  Because of the pattern, we know that the equilibrium constant gets smaller as more heat is added.  That means, the reaction is shifted to the left, towards the reactant side.  By Le Chatelier's principle, then, we know that the reaction is exothermic because when you apply stress (heat), the equilibrium relieves this heat by going to the reactant side, using up the heat.  Therefore, Delta H is negative.