Question

Tutored Practice Problem 16.4.1 C TO Predict and calculate the effect of concentration changes on an equilibrium system Close Problem Some COCl is allowed to dissociate into CO and Cl, at 873 K At equilibrium (COC) = 0.331 M. and (CO) = [C] -0.127 M. Additional [CO 0.224 M and the system is allowed to once again reach equilibrium is added so that COCI(8) CO() + CHCE) 6.98 102 at 873K (a) in which direction will the reaction proceed to reach equilibrium? (b) What are the new concentrations of reactants and products after the system reaches equilibrium? [COCI] [CO) (C12] 22

Answer 1

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Griven [coci2] = 0.231M , [co] - [[12] = 0.127M we are adding [co], according to Le-chatelier's principle reaction moves backward or shift Left side as concentration of product increase so to keep ke constant reaction moves backward, so I(M) C(M) [co] new = 0.22474 Coco + Cl2G - COClz (9) 0.224 0.127 0.231 -x -x tx 0.224-2 0-127-2 0.231+ ECM) kc becomes l _ - 1433 6.98x10-2 kc [cool] [co] [cz] 01231+X (0.224-^) (0-129-x) 14-33 = 0.231 +2 0.02 8445-0.224-0.1271 +2 14-33 = 0.231 + 0.028 449 -0.3512 + x2 0.41 - 5.03X + 14.33x2 = 0.231 + 0.179 - 6-02+14.33x2 a on solving value of a x =0.0321 [col= 0.224 -2 = 0.224 -0.0321 = 0.1919 M 0.0943M LC1273 0.127-a -0.127-0.0321 = Icoaz s 0.231 +2 = 0.231 +0.0321 = 0.2631 M.