Compounds ' $A$ ' and ' $B$ ' react according to the following chemical equation.
$$\mathrm{A}(\mathrm{~g})+2 \mathrm{~B}(\mathrm{~g}) \longrightarrow 2 \mathrm{C}(\mathrm{~g})$$
Concentration of either ' $A$ ' or ' $B$ ' were changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.
| Expereiment | Initial concentration of [A]/mol L$^{-1}$ |
Initial concentration of [B]/mol L$^{-1}$ |
Initial concentration of [C]/mol L$^{-1}$ S$^{-1}$ |
|---|---|---|---|
| 1. | 0.30 | 0.30 | 0.10 |
| 2. | 0.30 | 0.60 | 0.40 |
| 3. | 0.60 | 0.30 | 0.20 |
Which of the following statement is not correct for the catalyst?
The value of rate constant of a pseudo first order reaction ............ .
Consider the reaction $\mathrm{A} \longrightarrow \mathrm{B}$. The concentration of both the reactants and the products varies exponentially with time. Which of the following figures correctly describes the change in concentration of reactants and products with time?
Rate law cannot be determined from balanced chemical equation if ............... .