question_answer

Given the reaction between two gases represented by \[{{A}_{2}}\] and \[{{B}_{2}}\] to give the compound \[AB.(g).\]\[{{A}_{2}}(g)+{{B}_{2}}(g)2AB(g)\]

At equilibrium, the concentration of \[{{A}_{2}}=3.0\times {{10}^{-3}}M\] of \[{{B}_{2}}=4.2\times {{10}^{-3}}M\] of \[AB=2.8\times {{10}^{-3}}M\]. If the reaction takes place in a sealed vessel at \[527{}^\circ C,\] then the value of K, will be                                                                                                 [AIPMT (M) 2012]

A)  2.0              

B)  1.9                  

C)  0.62                

D)       4.5

Correct Answer: C

Solution :

The equilibrium constant is given by