The equilibrium constant, K c , for the reaction of iodine bromide to form iodine and bromine is 2.5× 10 −3 . If an equilibrium mixture contains 0.31 M IBr and 5.0× 10 −2 M I 2 , what is the molar concentration of B r 2 ? 2IBr(g)⇌ I 2 (g)+B r 2 (g)
2 IBr (g) I2 (g) + Br2 (g)
Equolibrium constant (Kc ) = (1)
Given, Kc = 2.5*10-3 ,
at equilibrium [IBr] =0.31 M, [I2] = 5.0*10-2 M
Putting the values in Eq.1
2.5*10-3 = 5.0*10-2 * [Br2] / (0.31)2
Or, [Br2] = { 2.5*10-3 *(0.31)2} ÷ {5.0*10-2 }
Or, [Br2] = 4.81 *10-3 M.
Hence, molar concentration of Br2= 4.81*10-3 M.
The equilibrium constant, K c , for the reaction of iodine bromide to form iodine and...
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