At equilibrium, a 4.50 L container has 2.6 g of carbon, CO2 at a partial pressure of 0.0020 atm, and a total pressure of 0.572 atm. Calculate KP for this reaction at 725oC.

The given question is incomplete.. The complete question is :

Consider the following reaction:

At equilibrium, a 4.50 L container has 2.6 g of carbon, CO2 at a partial pressure of 0.0020 atm, and a total pressure of 0.572 atm. Calculate KP for this reaction at 725oC.

162.45

Explanation:

Equilibrium pressure of = 0.0020 atm

Total pressure at equilibrium = 0.572 atm

Equilibrium pressure of = Total pressure at equilibrium - Equilibrium pressure of =  (0.572- 0.0020) = 0.570 atm

The given balanced equilibrium reaction is,

At eqm               0        0.0020        0.570

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

By solving we get :

Thus for this reaction at is 162.45

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.