The rate of an acid-catalyzed reaction in aqueous solution follows the rate equation r=k [X+ ] [Y2- ] [H+ ] If k16 and k4 are rate constants for the reaction at ionic strength of 16 mol L-1 and 4 mol L-1, respectively k4k16, in terms of Debye-Huckel constant (B=0.51), is

ABC26PH0938 · Chemical Kinetics

Subject: Physical Chemistry · Chapter: Chemical Kinetics · Topic: Rate Laws Order · Exam: NET DEC 2016 · Marks: 2 · Difficulty: Medium

The rate of an acid-catalyzed reaction in aqueous solution follows the rate equation

\[ \mathrm{r}=\mathrm{k}\left[\mathrm{X}^{+}\right]\left[\mathrm{Y}^{2-}\right]\left[\mathrm{H}^{+}\right] \]

If $\mathrm{k}_{16}$ and $\mathrm{k}_{4}$ are rate constants for the reaction at ionic strength of $16 \mathrm{mol} \mathrm{L}^{-1}$ and $4 \mathrm{mol} \mathrm{L}^{-1}$, respectively $\ln \frac{\mathrm{k}_{4}}{\mathrm{k}_{16}}$, in terms of Debye-Huckel constant $(\mathrm{B}=0.51)$, is

(a)4B

(b)8B

(c)10B

(d)12B

Answer

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Explanation

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