An investigation is conducted to study the kinetics of the reaction represented below:

\[ \text{A(aq)} + \text{B(aq)} \rightarrow \text{C(aq)} + \text{D(aq)} \]

The reaction is first order with respect to \(\text{A}\) and first order with respect to \(\text{B}\). Four separate trials are carried out under different experimental conditions, and the initial rate of reaction is recorded for each trial as shown in the table below.

Trial	Temperature (\(\text{K}\))	Catalyst present	Initial \([\text{A}]\) (\(\text{M}\))	Initial \([\text{B}]\) (\(\text{M}\))	Initial rate (\(\text{M}\cdot\text{s}^{-1}\))
1	\(295\)	No	\(0.10\)	\(0.10\)	\(1.2 \times 10^{-4}\)
2	\(295\)	No	\(0.20\)	\(0.20\)	\(4.8 \times 10^{-4}\)
3	\(325\)	No	\(0.10\)	\(0.10\)	\(6.0 \times 10^{-4}\)
4	\(325\)	Yes	\(0.10\)	\(0.10\)	\(3.6 \times 10^{-3}\)

Which of the following correctly ranks the rate constants, \(k_1\), \(k_2\), \(k_3\), and \(k_4\), for the four trials from greatest to least?