Half life of zero order reaction $A \rightarrow \text{product}$ is $1 \ \text{hour}$,when initial concentration of reactant is $2.0 \ \text{mol L}^{-1}$. The time required to decrease concentration of $A$ from $0.50$ to $0.25 \ \text{mol L}^{-1}$ is:

The half-life of a zero-order reaction is $1 \text{ hour}$. If the initial concentration of the reactant is $2.0 \text{ mol L}^{-1}$, find the time required to decrease the concentration from $0.50 \text{ mol L}^{-1}$ to $0.25 \text{ mol L}^{-1}$. (in $\text{ hour}$)

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

Calculate the rate constant of a zero order reaction if it is $90 \%$ completed in $90 \ s$.

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

What is the concentration (in $mol \ L^{-1}$) of the product $B$ after $20 \ s$ in the following reaction? Given that $A \longrightarrow 3B$,rate $= k[A]^0$. The data is provided in the table below:
| Time $(s)$ | Concentration of reactant $A$ $(mol \ L^{-1})$ |
| :--- | :--- |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |