2.50 moles of NOCl were placed in a 2.50 L reaction vessel at400deg cel. After e

Question

2.50 moles of NOCl were placed in a 2.50 L reaction vessel at400deg cel. After equilibrium was established, it was found that28% of the NOCl had dissaciated to the equation:                      2NOCl(g)<---> 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for this reaction. 2.50 moles of NOCl were placed in a 2.50 L reaction vessel at400deg cel. After equilibrium was established, it was found that28% of the NOCl had dissaciated to the equation:                      2NOCl(g)<---> 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for this reaction.

Explanation / Answer

We Know that :       The given Reaction is :         2NOCl(g)<---> 2NO(g) + Cl2(g)    I : 2.5                           0          0    C :  2 ( -0.28 )          +2 ( 0.28 )     +0.28     E:    0.776M              0.224 M        0.112 M                                                                              Kc = 0.112 x ( 0.224 ) 2 / (0.776 ) 2                                                                                       = 0.009332                                                                                          = 0.009332   

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