For the following reaction: $NO_2(g) + CO(g) \to NO(g) + CO_2(g)$, the rate law is: Rate $= k \,[NO_2]^2$. If $0.1\,mole$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?

For reaction :

$2NO_2(g) + O_3(g) \to N_2O_5(g) + O_2(g)$

rate law is $R = K\, [NO_2]' [O_3]'$.

Which of these possible reaction mechanisms is consistent with the rate law?

Mechanism $I :$

$NO_2(g) + O_3(g) \to NO_3(g) + O_2(g)$ (slow)

$NO_3(g) + NO_2(g) \to N_2O_5(g)$ (fast)

Mechanism $II :$

$O_3(g)  \rightleftharpoons  O_2(g) + [O]$ (fast)

$NO_2(g) + [O] \to NO_3$ (slow)

$NO_3(g) + NO_2(g) \to  N_2O_5$ (fast)

Write the rate equation for the reaction $2A + B\to C$ if the order of the reaction is zero.

Which of the following is the fastest reaction

For a reaction $X + Y \to Z$, rate $ \propto \, [X]$. What is $(i)$ molecularity and $(ii)$ order of reaction ?

 $A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$  but it is independent of the concentration of $B$, then