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InterviewSolution
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During the kinetic study of the reaction , `2A + B to C+ D ,` following results were obtained Based on the above date which one of the following is correct ?A. `Rate =k[A]^(2)[B]`B. `Rate =K[A][B}`C. `Rate k [A]^(2) [B]^(2)`D. `Rate =k [A][B]^(2)` |
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Answer» Correct Answer - D Let the of reaction with respect to A is x and with respect to B is Y thus , rate `=k|a|^(X)|B|^(y)` ( x and y are stoichiometric coefficient ) for the given cases , `I, Rate=K(0,1)^(X)(0,1)^(y) =6.0xx10^(-3)` `II. rate =K (0,3)^(X)(0.2)^(y)=7.2xx10^(-2)` `III. rate =K(0.3)^(X)(0.40)^(y)=2.88xx10^(-1)` `IV, rate = K(0,4)^(X) (0.1) ^(y) =2.40xx10^(-2)` dividing Eq. (i) by Eq.(iv) we get `((0.1)/(0.4))^(X)((0.1)/(0.1))^(Y)=(6.0xx10^(-3))/(2.4xx10^(-2))` `or ((1)/(4))^(x)=((1)/(4))^(1)` ` therefore x=1` On dividing Eq.(II) by Eq.(ii) we get `((0.3)/(0.3))^(x)((0.2)/(0.4))^(y)=(7.2xx10^(-2))/(2.88xx10^(-1))` `or ((1)/(2))^(y)=(1)/(4)` `or ((1)/(2))^(y) =((1)/(2))^(2)` `therefore y=2` thus rata law is , rate = `K[A]^(1) [B]^(2)` `=k|A|[B]^(2)` |
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