The rate of a gaseous reaction is given by the expression $k[A][B]^{2}$. If the volume of the vessel is reduced to one-half of the initial volume,the reaction rate as compared to the original rate is:

Velocity constant $K$ of a reaction is affected by

Consider the following reaction $A + B \rightarrow C$.
The time taken for $A$ to become $1/4$ of its initial concentration is twice the time taken to become $1/2$ of the same. Also,when the change of concentration of $B$ is plotted against time,the resulting graph gives a straight line with a negative slope and a positive intercept on the concentration axis. The overall order of the reaction is . . . . .

The rate law for the reaction $A + 2B \rightarrow C + 2D$ is given by:

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. How many times the rate of reaction is affected on increasing the concentration of $B$ three times?

Explain pseudo first order reaction by giving an example.