The equilibrium constant for Br2 + Br <-> Br3 at 25 degrees is 18. Calculate the equilibrium constant Br3 <-> Br2 + Br
eqn 1 Br2 + Br <-> Br3
eqn 2 Br3 <-> Br2 + Br
Equation 2 is the reverse of equation 1.
If k1 is 18, then k2 is 1/18.
To calculate the equilibrium constant for the reaction Br3 ↔ Br2 + Br, we can use the principle of the equilibrium constant expression and the relationship between the forward and reverse reactions.
Given that the equilibrium constant for the reaction Br2 + Br ↔ Br3 is 18, we can write the equilibrium constant expression as follows:
K1 = [Br3]/([Br2] × [Br])
Now, let's consider the reverse reaction Br3 ↔ Br2 + Br. According to the principle of the equilibrium constant expressions, the equilibrium constant for the reverse reaction in terms of the forward reaction can be calculated by taking the reciprocal of the equilibrium constant:
K2 = 1/K1
Substituting the given value of K1 into the equation:
K2 = 1/18
Therefore, the equilibrium constant K2 for the reaction Br3 ↔ Br2 + Br is approximately 0.056 (1/18).
To calculate the equilibrium constant for the reverse reaction, we can use the relationship between the forward and reverse equilibrium constants:
K_reverse = 1 / K_forward
In this case, the given forward equilibrium constant (K_forward) is 18. Therefore, we can calculate the equilibrium constant for the reverse reaction (K_reverse) as follows:
K_reverse = 1 / 18
≈ 0.0556
So, the equilibrium constant for the reaction Br3 <-> Br2 + Br is approximately 0.0556.
It is important to note that the given equilibrium constant (18) is a dimensionless quantity. The concentration unit for Br2, Br, and Br3 should be the same in both the forward and reverse reactions to use this relationship.