112g 2 Consider the dissociation of iodine we kno molecul 1

) 112g 2) Consider the dissociation of iodine: we kno molecul 12(8)- 21(g) f omic m A 1.00-g sample of I2 is heated to 1473 K in a 0.500-L flask. At equilibrium the total the number of moles for l2 at equilibrium and the equilibrium constant Ke. (Hint: the molar mass of l - 253.8 g/mol) l toces nlace in a single elementary step:

Solution

initial pressure of I2 (P) = nRT/V

           = (1/253.8)*0.0821*1473/0.5

           = 0.953 atm

        I2(g) <====> 2I(g)

initial 0.953         0

change    - x          2x

equili   0.953-x       2x

total pressure = 0.953-x+2x = 1.51 atm

x = 0.557

kp = pI^2/pI2

    = (2*0.557)^2/(0.953-0.557)

    = 3.134

kp = kc*(RT)^Dn

3.134 = x*(0.0821*1473)^1

x = Kc = 0.026