A mixture of 0.600 mol of bromine and 1.600 mol of iodine isplaced into a rigid

Question

A mixture of 0.600 mol of bromine and 1.600 mol of iodine isplaced into a rigid 1.000L container at 350 degrees celsius. Br2 (g) + I2 (g) --> 2 IBr (g)                        <-- When the mixture has come to equilibrium, the concentration ofiodine monobromide is 1.190 M. What is the equilibriumconstant forthis reaction at 350 degrees celsius? A mixture of 0.600 mol of bromine and 1.600 mol of iodine isplaced into a rigid 1.000L container at 350 degrees celsius. Br2 (g) + I2 (g) --> 2 IBr (g)                        <-- When the mixture has come to equilibrium, the concentration ofiodine monobromide is 1.190 M. What is the equilibriumconstant forthis reaction at 350 degrees celsius?

Explanation / Answer

Set up a RICE table. Br2     +       I2    2 IBr 0.600      1.600           0 -x               -x           +2x    ?   ?           1.190 2x = 1.190 x = 0.595 [Br2] = 0.600 -x                                               = 0.600 -0.595          = 0.005 [I2] = 1.600 - x       = 1.600 - 0.595       = 1.005 K = [IBr]2/[Br2][I2] K = (1.1902)/(0.005)(1.005) K = 281.81

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