The rate law for the reaction below is given by the expression $k\left[ A \right]\left[ B \right]$ 

                                          $A + B \to$ Product 

If the concentration of $B$ is increased from $0.1$ to $0.3\, mole$, keeping the value of $A$ at $0.1\, mole$, the rate constant will be

For the reaction $A + 2B \to C,$ rate is given by $R$ $ = [A]{[B]^2}$ then the order of the reaction is

The rate constant for the reaction $2N_2O_5 \to  4NO_2 + O_2$ is $3.0\times10^{-5}\, sec^{-1}$. If rate is $2.40\times10^{-5}\, M\, sec^{-1}$, then the concentration of $N_2O_5$ (in $M$) is ?

Write unit of rate constant of following reaction :

$1.$ $\frac {5}{2}$ order

$2.$  $n$ order

Select the rate law that corresponds to the data shown for the following reaction $A+ B\to C$

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.