For the reaction : $2A + B \to  A_2B$ ; the rate $= K[A]\, [B]^2$ with $K = 2.0\times10^{-6}\, lit^2\, mol^{-2}\, sec^{-1}$. Initial concentration of $A$ and $B$ are $0.2\, mol/lit$ and $0.4\, mol/lit$ respectively. Calculate the rate of reaction after $[A]$ is reduced to $0.12\, mol/litre$.

The incorrect order indicated against the rate of reaction is Rate Order

$A+B\xrightarrow{K}C$

Rate                        Order

The formation of gas at the surface of tungsten due to adsorption is the reaction of order

The rate constant of the reaction $2H_2O_2(aq) \to  2H_2O(aq) + O_2(g)$ is $3\times10^{-3}\, min^{-1}$. At what concentration of $H_2O_2$, the rate of reaction will be $2\times10^{-4}\, M\, s^{-1}$ ? ............ $M$

In a reaction $2A + B \to {A_2}B$, the reactant $ A $ will disappear at

The half life of forward and reverse reactions are $400\,\,sec$ and $100\,\,sec$ and these half lives are independent from the concentration of Reactant then find the equilibrium constant of the reaction