From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant: $(iv) \ C_{2}H_{5}Cl_{(g)} \rightarrow C_{2}H_{4(g)} + HCl_{(g)} \quad \text{Rate} = k[C_{2}H_{5}Cl]$

(A) Given rate expression is $\text{Rate} = k[C_{2}H_{5}Cl]^1$.
Since the exponent of the concentration term $[C_{2}H_{5}Cl]$ is $1$,the order of the reaction is $1$.
The dimension of the rate constant $k$ is calculated as:
$k = \frac{\text{Rate}}{[C_{2}H_{5}Cl]} = \frac{\text{mol} \ L^{-1} \ s^{-1}}{\text{mol} \ L^{-1}} = s^{-1}$.