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 a reaction $\mathrm{A} \xrightarrow{\mathrm{K}_4} \mathrm{~B} \xrightarrow{\mathrm{K}_2} \mathrm{C}$

If the rate of formation of $B$ is set to be zero then the concentration of $B$ is given by :

The reaction $2FeC{l_3} + SnC{l_2} \to 2FeC{l_2} + SnC{l_4}$ is an example of

The rate law for the reaction  Sucrose + Water $\xrightarrow{{[{H^ + }]}}$ Glucose + Fructose is given by

What is the order of reaction $r\, = \,k{[A]^{\frac{3}{2}}}\,{[B]^2}$ ?

Identify the reaction order from each of the following rate constants.

$(i)$ $k=2.3 \times 10^{-5} \,L \,mol ^{-1}\, s ^{-1}$

$(ii)$ $k=3 \times 10^{-4}\, s ^{-1}$