- A$C{H_3}C{H_2}OH$
- B${C_6}{H_5}OH$
- ✓$C{H_3}COOH$
- D$C{H_3}C{H_2}C{H_2}OH$
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$\mathop {\begin{array}{*{20}{c}}
{O\,\,\,\,\,\,\,\,\,\,\,\,\,} \\
{||\,\,\,\,\,\,\,\,\,\,\,\,} \\
{C{H_3} - C - C{H_2} - Cl}
\end{array}}\limits_{\left( I \right)} $ $\underset{(II)}{\mathop{\begin{matrix}
\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,O \\
\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,||\,\,\, \\
Cl-C{{H}_{2}}-C-H \\
\end{matrix}}}\,$
$\mathop {\begin{array}{*{20}{c}}
O \\
{||} \\
{H - C - H}
\end{array}}\limits_{\left( {III} \right)} $ $\mathop {\begin{array}{*{20}{c}}
O \\
{||} \\
{{H_3}C - C - C{H_3}}
\end{array}}\limits_{\left( {IV} \right)} $
The half-life period is independent of the concentration of zinc at constant $pH$. For the constant concentration of $Zn$, the rate becomes $100$ times when $pH$ is decreased from $3\, to\, 2$. Identify the correct statements $(pH = -\log [H^{+}])$
$(A)$ $\frac{{dx}}{{dt}}\, = k{[Zn]^0}{[{H^ + }]^2}$
$(B)$ $\frac{{dx}}{{dt}}\, = k{[Zn]}{[{H^ + }]^2}$
$(C)$ Rate is not affected if the concentraton of zinc is made four times and that of $H^+$ ion is halved.
$(D)$ Rate becomes four times if the concentration of $H^+$ ion is doubled at constant $Zn$ concentration