he equilibrium constant, Kc, for the reaction:2 NOCl (g) 2 NO (g) + Cl2 (g) is 2.4 x 10 -7What is the equilibrium constant, Kc, for the reaction:1/3 Cl2 (g ) + 2/3 NO (g) 2/3 NOCl (g
Question
he equilibrium constant, Kc, for the reaction:2 NOCl (g) 2 NO (g) + Cl2 (g) is 2.4 x 10 -7What is the equilibrium constant, Kc, for the reaction:1/3 Cl2 (g ) + 2/3 NO (g) 2/3 NOCl (g
Solution
The equilibrium constant for a reaction is related to the stoichiometry of the reaction. If we reverse the reaction, the equilibrium constant becomes the reciprocal of the original. If we multiply the reaction by a factor, the equilibrium constant is raised to that power.
The original reaction is: 2 NOCl (g) ⇌ 2 NO (g) + Cl2 (g) with Kc1 = 2.4 x 10^-7
The new reaction is: 1/3 Cl2 (g) + 2/3 NO (g) ⇌ 2/3 NOCl (g)
This new reaction is the original reaction reversed and multiplied by 1/3.
So, to find the new equilibrium constant, we take the reciprocal of the original (because the reaction is reversed) and then raise it to the power of 1/3 (because the reaction is multiplied by 1/3).
Kc2 = (1/Kc1)^(1/3)
Substitute the given value of Kc1 into the equation:
Kc2 = (1/(2.4 x 10^-7))^(1/3)
Calculate the reciprocal:
Kc2 = (4.17 x 10^6)^(1/3)
Finally, calculate the cube root:
Kc2 = 160.6
So, the equilibrium constant, Kc, for the reaction: 1/3 Cl2 (g) + 2/3 NO (g) ⇌ 2/3 NOCl (g) is approximately 160.6.
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