The rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.

Consider the following single step reaction in gas phase at constant temperature.
$2 \ A_{(g)} + B_{(g)} \rightarrow C_{(g)}$
The initial rate of the reaction is recorded as $r_1$ when the reaction starts with $1.5 \ atm$ pressure of $A$ and $0.7 \ atm$ pressure of $B$. After some time,the rate $r_2$ is recorded when the pressure of $C$ becomes $0.5 \ atm$. The ratio $r_1 : r_2$ is $\qquad$ $\times 10^{-1}$.
(Nearest integer)

For a reaction,$A + B \longrightarrow \text{product}$,it is found that the rate law is $r = k[A]^{1.5}[B]^{2.5}$. What is the order of reaction?

The rate constants for first-order and second-order reactions have units of ..... respectively.

The following reactions occur for the reaction of $NO$ with $Br_2$ to form $NOBr$:
$NO_{(g)} + Br_{2_{(g)}} \rightleftharpoons NOBr_{2_{(g)}}$
$NOBr_{2_{(g)}} + NO_{(g)} \rightarrow 2 NOBr_{(g)}$
If the second reaction is the rate-determining step,the order of the reaction with respect to $NO_{(g)}$ will be:

Select the incorrect option :