$A$ reaction $2A + B \xrightarrow{k} C + D$ is first order with respect to $A$ and second order with respect to $B$. Initial concentration $(t = 0)$ of $A$ is $C_0$ while $B$ is $2C_0$. If at $t = 30 \min$ the concentration of $C$ is $C_0/4$,then the rate expression at $t = 30 \min$ is:

Inversion of cane sugar is an example of $-$

$t_{1/2} =$ constant confirms a first-order reaction. If $a^2 t_{1/2} =$ constant,it confirms that the order of the reaction is ($a =$ initial concentration of reactant).

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

The reaction rate between two substances $A$ and $B$ is expressed as: $\text{rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the ratio of the new rate to the initial rate will be:

Consider the following reaction $A + B \rightarrow C$.
The time taken for $A$ to become $1/4$ of its initial concentration is twice the time taken to become $1/2$ of the same. Also,when the change of concentration of $B$ is plotted against time,the resulting graph gives a straight line with a negative slope and a positive intercept on the concentration axis. The overall order of the reaction is . . . . .