At 350 K, Kc = 0.142 for the reaction
2 BrCl(g) ⇀↽ Br2(g) + Cl2(g)
An equilibrium mixture at this temperature contains equal concentrations of bromine and chlorine, 0.077 mol/L. What is the equilibrium concentration of BrCl?
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To find the equilibrium concentration of BrCl, we can use the equilibrium constant expression for the reaction, Kc = [Br2][Cl2]/[BrCl]^2.
Given that the equilibrium constant (Kc) is 0.142 and the concentrations of bromine (Br2) and chlorine (Cl2) are both 0.077 mol/L, we can substitute these values into the equilibrium constant expression as follows:
0.142 = (0.077)(0.077)/[BrCl]^2
Simplifying the equation:
0.142 = 0.005929/[BrCl]^2
Now, we can rearrange the equation to solve for [BrCl]^2:
[BrCl]^2 = 0.005929/0.142
[BrCl]^2 ≈ 0.041698
Taking the square root of both sides of the equation:
[BrCl] ≈ √0.041698
[BrCl] ≈ 0.204 mol/L
Therefore, the equilibrium concentration of BrCl is approximately 0.204 mol/L.