Seema Saini Solutions for Chapter: Chemical Kinetics, Exercise 6: DPP 4.6

Acid hydrolysis of the ester is the first-order reaction, and rate constant is given by
$\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{{\mathrm{V}}_{\infty }-{\mathrm{V}}_0}{{\mathrm{V}}_{\infty }-{\mathrm{V}}_{\mathrm{t}}}$,
where ${\mathrm{V}}_{\mathrm{t}}, {\mathrm{V}}_0$ and ${\mathrm{V}}_{\infty }$ are the volume of standard $\mathrm{NaOH}$ needed to neutralize acid present at a given time. If ester is $50\%$ neutralised then

Inversion of sucrose $\left({\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\right)$ is the first-order reaction and is studied by measuring the angle of rotation at different intervals of time
.
If $\left({\mathrm{r}}_{\infty }-{\mathrm{r}}_0\right)\equiv \mathrm{a}$ and $\left({\mathrm{r}}_{\infty }-{\mathrm{r}}_{\mathrm{t}}\right)\equiv (\mathrm{a}-\mathrm{x}),$ (where, ${\mathrm{r}}_0, {\mathrm{r}}_1$ and ${\mathrm{r}}_{\infty }$ are the angles of rotation at the start, at the time $\mathrm{t}$ and at the end of the reaction, respectively), then there is $50\%$ inversion when:

Saponification of ethyl acetate $\left({\mathrm{CH}}_3{\mathrm{COOC}}_2{\mathrm{H}}_5\right)$ by $\mathrm{NaOH}$ is studied by titration of the reaction mixture having $1:1$ molar ratio of the reactants. If $10 \mathrm{mL}$ of $1\mathrm{N} \mathrm{HCl}$ is required by $5 \mathrm{mL}$ of the solution at the start and $8 \mathrm{ml}$of $1\mathrm{N} \mathrm{HCl}$ is required by another $5 \mathrm{mL}$ after $10$ minutes, then the rate constant is-

Consider the decay of $\mathrm{P}$ to $\mathrm{A}$ and $\mathrm{B}$ by two parallel first-order reactions as shown in the figure

Which of the following is (are) true?

Which of the following statements are correct?

In the reversible reaction, ${\text{2NO}}_2\underset{{\mathrm{k}}_2}{\overset{{\mathrm{k}}_1}{\rightleftharpoons }}{\mathrm{N}}_2{\mathrm{O}}_4,$ the rate of disappearance of ${\mathrm{NO}}_2$ is equal to-

The rate expression for the reaction,

${\mathrm{NH}}_4\mathrm{CNO}\stackrel{\mathrm{k}}{\to }{\mathrm{NH}}_2{\mathrm{CONH}}_2$

can be derived from the mechanism,

$\left(\mathrm{i}\right)$ ${\mathrm{NH}}_4\mathrm{CNO}\underset{{\mathrm{k}}_2}{\overset{{\mathrm{k}}_1}{\rightleftharpoons }}{\mathrm{NH}}_4\mathrm{NCO} \left(\mathrm{Fast}\right)$

$\left(\mathrm{ii}\right)$ ${\mathrm{NH}}_4\mathrm{NCO}\stackrel{{\mathrm{k}}_3}{⟶}{\mathrm{NH}}_3+\mathrm{HNCO} \left(\mathrm{Fast}\right)$

$\left(\mathrm{iii}\right)$ ${\mathrm{NH}}_3+\mathrm{HNCO}\stackrel{{\mathrm{k}}_4}{⟶}{\mathrm{NH}}_2{\mathrm{CONH}}_2 \left(\mathrm{Slow}\right)$

Which of the following statements are correct about rate expression?

The rate of formation of ${\mathrm{C}}_6{\mathrm{H}}_6+3{\mathrm{H}}_2\underset{{\mathrm{k}}_{\mathrm{b}}}{\overset{{\mathrm{k}}_{\mathrm{f}}}{\rightleftharpoons }}{\mathrm{C}}_6{\mathrm{H}}_{12}$ for the forward reaction, is first-order with respect to ${\mathrm{C}}_6{\mathrm{H}}_6$ and ${\mathrm{H}}_2$ each. Which among the following are correct?