Consider the plots for the types of reaction $nA \to B + C$. These plots respectively correspond to the reaction orders:

$100 \text{ cm}^3$ of $1 \text{ M } CH_3COOH$ was mixed with $100 \text{ cm}^3$ of $2 \text{ M } CH_3OH$ to form an ester. The change in the initial rate if each solution is diluted with an equal volume of water would be: (in $\text{times}$)

Which among the following is a false statement?

If the reaction between $A$ and $B$ to give $C$ shows first-order kinetics in $A$ and second-order in $B$,the rate equation can be written as:

Identify the reaction order for which the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$.

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)