Question $1$:

The liquid$-$phase reaction

Trityl $($A$)+$ Methanol $($B$)$ Products $($C$)$

was carried out in a batch reactor at $25C$ in a solution of benzene and pyridine in an excess of methanol $($:$mo\frac{l}{d}{m}^3\}.$ Pyridine reacts with $HCl,$ which then precipitates as pyridine hydro$-$chloride thereby making the reaction irreversible. The reaction is first order in methanol. The concentration of triphenyl methyl chloride $($A$)$ was measured as a function of time and is shown below:

$\backslash$table$[[$TABLE E$7-1\mathrm{.}1,$RAW DATA,,,,,,$],[t(min),0,50,100,150,200,250,300],[C_A(mo\frac{l}{d}{m}^3),0\mathrm{.}05,0\mathrm{.}038,0\mathrm{.}0306,0\mathrm{.}0256,0\mathrm{.}0222,0\mathrm{.}0195,0\mathrm{.}0174]]$

Use the integral method to confirm that the reaction is second order and if yes calculate the reaction rate constant.

Hint: When you have excess amount, it can be considered constant.

Question $2$

$A+BC+D$

Using the data from question$1$ determine the reaction order with respect to $A.$