For a certain reaction the expression for half life is $t \propto \frac{1}{{{a^{n - 1}}}}$ then the order of reaction is

The reaction $CH _{3} COF + H _{2} O \quad \rightleftharpoons CH _{3} COOH + HF$

Condition $I$ $:$ $\left[ H _{2} O \right]_{0}=1.00 \,M$

                           $\left[ CH _{3} COF \right]_{0}=0.01 \,M$

Condition $II$ $:$ $\left[ H _{2} O \right]_{0}=0.02 \,M$

                             $\left[ CH _{3} COF \right]_{0}=0.80 \,M$

Determine the order of reaction and calculate rate constant.

Differential form of the rate equation is

$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$

Which statement about the above equation is wrong?

Which of the following oxides of nitrogen will be the most stable one

Certain bimolecular reactions which follow the first order kinetics are called

The following mechanism has been proposed for the reaction of $NO$ with $Br_2$ to form $NOBr$ :

$NO(g) + Br_2 (g) \rightleftharpoons NOBr_2 (g)$

$NOBr_2(g)+ NO(g) \longrightarrow 2NOBr(g)$

If the second step is the rate determining step, the order of the reaction with respect to $NO(g)$ is