If the order of the reaction $x + y \xrightarrow{hv} xy$ is zero,it means that the rate of

For a reaction $r = k[A][B]^2$,if the concentration of $A$ is doubled,the rate of reaction:

For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

Write the general reaction and its rate law.

The rate of reaction $A + B \rightarrow P$ is $4 \times 10^{-2} \text{ mol dm}^{-3} \text{ s}^{-1}$. When $[A] = 0.2 \text{ mol dm}^{-3}$ and $[B] = 0.1 \text{ mol dm}^{-3}$, what is the rate constant of the reaction, if it is first order with respect to $A$ and second order with respect to $B$?

The rate for the reaction $A + B \rightarrow \text{product}$ is $1.8 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is second order in $A$ and first order in $B$,given $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$.