The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

With the help of an example,explain what is meant by a pseudo first order reaction.

For a chemical reaction $Y + 2Z \to$ Product,the rate-controlling step is $Y + \frac{1}{2}Z \to Q$. If the concentration of $Z$ is doubled,the rate of reaction will:

The reaction of formation of phosgene from $CO$ and $Cl_2$ is $CO + Cl_2 \to COCl_2.$ The proposed mechanism is
$(i)$ $Cl_2 \,\underset{k_2}{\overset{k_1}{\longleftrightarrow}}\, 2Cl$
$(ii)$ $Cl + CO \,\underset{k_4}{\overset{k_3}{\longleftrightarrow}}\, COCl$
$(iii)$ $COCl + Cl_2 \xrightarrow{k_5} COCl_2 + Cl$ (slow)
Find the correct expression of rate law.

In the reaction,$P + Q \longrightarrow R + S$,the time taken for $75 \%$ reaction of $P$ is twice the time taken for $50 \%$ reaction of $P$. The concentration of $Q$ varies with reaction time as shown in the figure. The overall order of the reaction is

Why can’t molecularity of any reaction be equal to zero?