Rate law for the reaction,$C_2H_5I_{(g)} \rightarrow C_2H_{4_{(g)}} + HI_{(g)}$ is $r = k[C_2H_5I]$. What is the order and molecularity of this reaction?

For the reaction $2A + B \rightarrow \text{Product}$,the half-life period remains unchanged when the concentration of $B$ is doubled. However,when the concentration of $A$ is doubled,the rate of the reaction doubles. Determine the unit of the rate constant for this reaction.

The following are the rate constants of two different reactions. What is the overall order of reaction for each?
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

For a hypothetical reaction $A + B \rightarrow C$,the following data is provided from three different experiments:
$1$. $[A] = 0.01 \ M$,$[B] = 0.01 \ M$ - Rate of reaction $= 1.0 \times 10^{-4} \ M \ s^{-1}$.
$2$. $[A] = 0.01 \ M$,$[B] = 0.03 \ M$ - Rate of reaction $= 9.0 \times 10^{-4} \ M \ s^{-1}$.
$3$. $[A] = 0.03 \ M$,$[B] = 0.03 \ M$ - Rate of reaction $= 2.70 \times 10^{-3} \ M \ s^{-1}$.
Determine the rate law.

$1 \ L$ of $2 \ M$ $CH_3COOH$ is mixed with $1 \ L$ of $3 \ M$ $C_2H_5OH$ to form an ester. The rate of the reaction with respect to the initial rate when each solution is diluted with an equal volume of water will be (in times).

The rate law for the reaction between substances $A$ and $B$ is given by $\text{Rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,what is the ratio of the new rate to the initial rate?