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Consider the following reaction at 1600°C:
When 1.05 moles Br2 are placed in a 2L flask, 2.50% of Br2 undergoes dissociation. Calculate Kp for the reaction.
Solution:
Consider the chemical reaction above
The first thing that we need to do is to get the molarity of Br2 as follows
At equilibrium, the amount of remaining Br2 is
At equilibrium, the amount of Br formed is
Hence, the equilibrium constant of the given reaction is
Since all products and reactants for the given reactions are all gases, then we have to use the formula as follows
where ∆n is the difference between the sum of the coefficients of the products and the sum of the coefficients of the reactants.
The universal gas law constant for gmole, atmosphere, liters, and K is
.
.The absolute temperature of the reaction is
Therefore, the value of Kp for the given reaction is
