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?

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 $A$ $(mol \ L^{-1})$ |
| :--- | :--- |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |

For a zero-order reaction $A \rightarrow \text{Product}$,the half-life is $1 \ h$. If the initial concentration of reactant $A$ is $2.0 \ mol \ L^{-1}$,how many hours will it take for the concentration to decrease from $0.50 \ mol \ L^{-1}$ to $0.25 \ mol \ L^{-1}$?

In the reaction,$A \rightarrow$ products,if the concentration of the reactant is doubled,the rate of the reaction remains unchanged. The order of the reaction with respect to $A$ is

The decomposition of $NH_3$ on a platinum surface is a zero-order reaction. What is the rate of production of $N_2$ if $k = 2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$?

Describe the nature of the following graphs for a zero-order reaction:
$(i)$ Concentration of reactant $\to$ Time
$(ii)$ Concentration of product $\to$ Time