Some COCl 2 is allowed to dissociate into CO and Cl 2 at 873 K. At equilibrium,

Question

Some COCl2 is allowed to dissociate into CO and Cl2 at 873 K. At equilibrium, [COCl2] = 0.255 M, and [CO] = [Cl2] = 0.133 M. Additional CO is added so that [CO]new = 0.235 M and the system is allowed to once again reach equilibrium.

COCl2(g) = CO(g) + Cl2(g) K = 6.98×10-2 at 873 K

(a) In which direction will the reaction proceed to reach equilibrium? _________to the rightto the left

(b) What are the new concentrations of reactants and products after the system reaches equilibrium?

Explanation / Answer

        COCl2(g) <----> CO(g) + Cl2(g)

equil     0.225 M        0.133 M 0.133 M

added to     ---         0.235 M ---   

re-equil 0.225+x        0.235-x   0.133-x

Kc = [Cl2]*[CO]/[COCL2]

a) direction of reaction proceeds = right to left

0.0698 = ((0.133-x)*(0.235-x))/(0.225+x))

x = 0.039

[COCL2] = 0.225+0.039 = 0.264 M

[Cl2] = 0.235-0.039 = 0.196 M

[CO] = 0.133-0.039 = 0.094 M

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