Give two examples of zero-order reactions and two examples of first-order reactions.

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)

In a reaction involving hydrolysis of an organic chloride in the presence of a large excess of water,$RCl + H_2O \to ROH + HCl$.

For the chemical reaction $2A + 2B + C \rightarrow \text{Product}$,the rate law is given by $r \propto [A] [B]^2$. What is the order of the reaction?

For the reaction $A \to xP$,when $[A] = 2.2 \, mM$,the rate was found to be $2.4 \, mM \, s^{-1}$. On reducing the concentration of $A$ to half,the rate changes to $0.6 \, mM \, s^{-1}$. The order of reaction with respect to $A$ is

Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. Which of the following conditions does $NOT$ affect the rate of reaction?