Read the Passage carefully and answer the Questions
Kinetic studies not only help us to determine the rate of a chemical reaction but also describe the conditions by which the reaction rates can be altered. The factors such as concentration, temperature, pressure and catalyst affect the rate of a reaction.
The speed of a reaction or the rate of a reaction can be defined as the change in concentration of a reactant or product in unit time.
Rate \(=k[A]^{\text {a }}[B]^{\text {y }}\)
Here \(k\) is the rate constant
\(x+y\) gives the overall order of a reaction, whereas \(x\) and \(y\) repreeent the order with respect to the reactants \(A\) and \(B\), respectively.
Table: Initial rate of formation of NO 2

S No.	Initial [NO]/mol L-1	Initial [O2]/mol L-1	Initial rate of formation of NO2/mol L-1s-1
1.	0.30	0.3	0.096
2.	0.60	0.3	0.384
3.	0.30	0.6	0.192
4.	0.60	0.6	0.768

1. A Rate of reaction \(=k[ NO ]^2\left[ O _2\right]\)
2. B Rate of reaction \(=k[ NO ]\left[ O _2\right]^2\)
3. C Rate of reaction \(=k[ NO ]^2\left[ O _2\right]^2\)
4. D Rate of reaction \(=k[ NO ]\left[ O _2\right]\)