A) At 1285 o C the equilibrium constant for thereaction Br 2(g) --> 2Br (g) isK

Question

A) At 1285 oC the equilibrium constant for thereaction Br2(g) --> 2Br(g) isKc= 1.04 x 10-3.
     A 0.200 L vessel containing an equilibriummixture of the gases has 0.245 g of Br2(g) in it.      What is the mass of Br(g)in the vessel? B) For the reaction H2(g) + I2(g) -->2HI(g), Kc= 55.3 at 700 K. In a 2.00 Lflask containing      an equilibrium mixture of the threegases, there are 0.056 g H2 and 4.36 gI2.      What is the mass of HI in theflask? A) At 1285 oC the equilibrium constant for thereaction Br2(g) --> 2Br(g) isKc= 1.04 x 10-3.
     A 0.200 L vessel containing an equilibriummixture of the gases has 0.245 g of Br2(g) in it.      What is the mass of Br(g)in the vessel? B) For the reaction H2(g) + I2(g) -->2HI(g), Kc= 55.3 at 700 K. In a 2.00 Lflask containing      an equilibrium mixture of the threegases, there are 0.056 g H2 and 4.36 gI2.      What is the mass of HI in theflask?

Explanation / Answer

First find the concentration of Br2 in the vessel. [Br2] = 0.245g x mol/159.8g = 0.00153mol/0.200L =0.0077M Kc = [Br]2/[Br2] 1.04 x 10-3 x 0.0077 = [Br]2 Br = 2.82 x 10-3mol/L x 0.200L = 0.000565mol x79.9g/mol = 0.0451g or 4.5 x 10-2g Part b Find the concentrations for H2 andI2. [H2] = 0.056g x mol/2.02g =0.0277mol/2L =0.0139M [I2] = 4.36g x mol/253.08g = 0.01723mol/2L=0.00861M kc = [HI]2/[I2][H2] 55.3 x 0.0139 x 0.00861 = [HI]2 [HI] = 0.0814mol/L x 2L = 0.1627mol x 127.914g/mol =20.8g Hope that helps [HI] = 0.0814mol/L x 2L = 0.1627mol x 127.914g/mol =20.8g Hope that helps

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