A system equilibrium at 25 degrees Celsius in a 1.0L container was found to cont

Question

A system equilibrium at 25 degrees Celsius in a 1.0L container was found to contain 0.0568 moles of BrCl, 0.0216 moles of Br2, and 0.0216 moles of Cl2. If 0.020 moles of BrCl is added to this system, determine the new equilibrium concentrations.

Explanation / Answer

We first have to find the Keq value from the given data 2BrCl ---> Br2 + Cl2 [BrCl] = 0.0568 M [Cl2] = 0.0216 M [Br2] = 0.0216 M Keq = [Br2][Cl2]/[BrCl]^2 Keq = 0.0216*0.0216/(0.0568^2) Keq = 0.1446 now when 0.02 moles of BrCl are added then let say x amt of them is reacted 2BrCl ---> Br2 + Cl2 [BrCl] = 0.2568 -2x M [Cl2] = 0.0216 + x M [Br2] = 0.0216 +x M Keq = [Br2][Cl2]/[BrCl]^2 0.1446 = (0.0216 +x)^2/(0.2568 -2x)^2 x = 0.04319 M therefore, [BrCl] = 0.2568 -2*0.04319 M = 0.17042 M [Cl2] = 0.0216 + 0.04319 M = 0.06479 M [Br2] = 0.0216 +0.04319 M = 0.06479 M

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