General Chemistry 2: Rates of Reaction

Consider a solution of 0.10 M H$^{+}$ in 0.10 M thioacetimide at 25 $^\circ$C

rate = k[H$^{+}$][CH$_3$CSNH$_2$]

How are the rate and the rate constant (k) effected when water is added to the solution? When the reaction is heated to 75$^\circ$C ? When NaOH is added?

Derive the rate law given the elementary steps.

$Cl_2~\mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~2~Cl~~{1}$

$Cl+~CHCl_3~\xrightarrow{k_2}~HCl~+~CCl_3~~{2}$

$Cl~+~CCl_3~\xrightarrow{k_3}~CCl_4~~{3}$

For the proposed mechanism below, identify the intermediates and determine the rate law.

$2~NO_2~+~F_2~\leftrightharpoons~2~NO_2F~~{overall}$

$NO_2F_2+~Br_2~\longrightarrow~NO_2F~+~F~~{slow step}$

$NO_2~+~F~\longrightarrow~NO_2F$

For the proposed mechanism below, find the overall reaction, identify the intermediates, then determine the rate law.

$CL_2~\leftrightharpoons~2~Cl$

$2~Cl~+2~NO~\longrightarrow~2~NOCl$