The results given in the below table were obtained during kinetic studies of the following reaction:
2A + B $\to$ C + D

X and Y in the given table are respectively :

1. 0.3, 0.4

2. 0.4, 0.3

3. 0.4, 0.4

4. 0.3, 0.3

For the reaction \(2 A+B \rightarrow C,\) the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is:

For the non – stoichiometry reaction 2A + B → C + D, the following kinetic data were obtained in three separate experiments (all at 298 K).

The rate law for the formation of C is:

1. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}{]}^2\right[\mathrm{B}]$

2. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right][\mathrm{B}{]}^2$

3. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]$

4. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]\left[\mathrm{B}\right]$

The time for the half-life period of a certain reaction A → Products is 1 hour. When the initial concentration of the reactant 'A' is 2.0 mol L^-1, the time taken for its concentration to come from 0.50 to 0.25 mol L^-1,if it is a zero-order reaction, is:

Consider the reaction, 2A + B → Products.
When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:

1. L mol^–1 s^–1

2. no unit

3. mol L^–1s^–1

4. s^–1

A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will: 

1. Remain unchanged 

2. Triple 

3. Increases by a factor of 4 

4. Double 

H₂ gas is absorbed on the metal surface like gold, tungsten, etc. This follows ________ order reaction: