Q81 · CSIR NET Chemistry, December 2016
Paper: CSIR NET December 2016 · Subject: Physical Chemistry · Chapter: Chemical Kinetics · Topic: Rate Laws Order · Marks: 2 · Difficulty: Medium
The rate of an acid-catalyzed reaction in aqueous solution follows the rate equation
$r = k[\mathrm{X^+}][\mathrm{Y^{2-}}][\mathrm{H^+}]$
If $k_{16}$ and $k_4$ are rate constants for the reaction at ionic strength of $16\ \mathrm{mol\,L^{-1}}$ and $4\ \mathrm{mol\,L^{-1}}$, respectively $\ln\frac{k_4}{k_{16}}$, in terms of Debye-Huckel constant $(B = 0.51)$, is(a)4B
(b)8B
(c)10B
(d)12B
Answer
SELF-PRACTICE — the source book printed no answer.
Nothing is invented here, so this question has no answer on record.
Explanation
No explanation was printed for this question.
Study loop for Chemical Kinetics