InterviewSolution
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InterviewSolution
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Compounds A and B react according to the following chemical equation : `A(g) + 2B(g) rarr2C(g)` Concentration of either A or B were changed keeping the concentrations of one of the reactant constants and rates were measured as a function of initial concentration, Following results were obtained. Choose the correct option for the rate equations for this reaction.A. Rate = `k[A]^(2)[B]`B. Rate = `k[A][B]^(2)`C. Rate = `k[A][B]`D. Rate = `k[A]^(2)[B]^(0)` |
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Answer» Correct Answer - B Let Rate law, `r=k[A]^(x)[B]^(y)" "....(i)` On putting values, we get `0.10 = K [0.30]^(x)[0.30]^(y) " "....(ii)` `0.40 = K[0.30]^(x)[0.60]^(y)" "....(iii)` `0.20=K[0.60]^(x)[0.30]^(y)" "....(iv)` From Eqs. (ii) and (iii), we get `(0.1)/(0.4)=[(0.30)/(0.30)]^(x)[(0.30)/(0.60)]^(y)` `(1)/(4)=[(1)/(2)]^(y)implies y = 2` From Eqs. (iii) and (iv), we get `(0.40)/(0.20)=((0.30)/(0.60))^(x)((0.60)/(0.30))^(y)` `2=((1)/(2))^(x)(2)^(y)` On putting the values of y, we get `2=((1)/(2))^(x)(2)^(2)` `implies " "x=1` On putting the values of x and y in Eq. (i), we get `r=k[A]^(1)[B]^(2)=k[A][B]^(2)` |
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