The equilibrium will change in the direction of the reactants. The equilibrium w

Question

The equilibrium will change in the direction of the reactants. The equilibrium will change in the direction of the products. No change in equilibrium is observed. The equilibrium constant will decrease. Consider the following reaction: COCl_2(g) = CO(g) + Cl_(g) A reaction mixture initially contains 1.6M COCl_2 Determine the equilibrium concentration of CO if K_c for the reaction at this temperatures 833 times 10^-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. 1.5 times 10^-3 M 1.3 times 10^-3 M 4.2 times 10^-4 M 2.1 times 10^-2 M 3.7 times 10^-2 M The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + B(g) = A_2B(g) K_c = ? A_2B(g) _ B(g) = A_2B_2(g) K_c = 16.4

Explanation / Answer

                                CoCl2                  Co                   Cl2

Initial                      1.6 M                   0                    0

Change                 -x                        +x                   x

Equilibrium      1.6-x                         x                   x

KC= [CO][Cl2]/[CoCl2] = x2/(1.6-x)= 8.33*10-4, when x is neglected in comparison with 1.6

Now x2= 8.33*10-4*1.6, x= [CO] = 0.037 ( E is the correct answer)

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