In the reaction $2A + B \to A_2B$,if the concentration of $A$ is doubled and the concentration of $B$ is halved,then the rate of the reaction will:

The rate of a certain reaction depends on concentration according to the equation $\frac{-dc}{dt} = \frac{K_1 C}{1 + K_2 C}$. What is the order of the reaction when the concentration $(C)$ is very high?

Rate law for a reaction is $r=k[A]^2[B]$. If rate constant is $6.25 \ mol^{-2} \ dm^6 \ s^{-1}$,what is the rate of reaction when $[A]=1 \ mol \ dm^{-3}$ and $[B]=0.2 \ mol \ dm^{-3}$?

Consider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?

For a given reaction $t_{1/2} = \frac{1}{Ka}$. The order of the reaction is

$A_{(g)} + 2B_{(g)} \to$ product is an elementary reaction. Which of the following is incorrect?