Integrated Rate Equations-Zero Order Reactions

The rate constant for a zero order reaction $\mathrm{A}\to$ products is $0.0030 \mathrm{mol} {\mathrm{L}}^{-1} {\mathrm{s}}^{-1}$. How long it will take for the initial concentration of $\mathrm{A}$ to fall from $0.10\mathrm{M}$ to $0.075\mathrm{M}$?

Which of the following curve represent zero order reaction of $\mathrm{A}\mathrm{ }\to \mathrm{ }$products?

Which of the following equations represent integrated rate equation of zero order reaction?

For a zero-order reaction, with the initial reactant concentration $\mathrm{a}$, the time for completion of the reaction is:

In the following reaction $\mathrm{A}\to \mathrm{B}+\mathrm{C}$ rate constant is $0.001 {\mathrm{Msec}}^{–1}$. If we start with $1\mathrm{M}$ of $\mathrm{A}$ then concentration of $\mathrm{A}$ and $\mathrm{B}$ after $10$ minutes are :

In the reaction, $\mathrm{P}+\mathrm{Q}\to \mathrm{R}+\mathrm{S}$
The time taken for 75% reaction of P is twice the time taken for 50% reaction of P. The concentration of Q varies with reaction time as shown in the figure. The overall order of the reaction is

The reaction $2X\to B$ is a zeroth order reaction. If the initial concentration of $X$ is $0.2 M$, the half-life is $6h$. When the initial concentration of $X$ is $0.5M$, the time required to reach its final concentration of $0.2M$ will be:

Which of the following curve represent zero order reaction of $\mathrm{A}\mathrm{ }\to \mathrm{ }$products?

Which of the following curve represent zero order reaction of $\mathrm{A}\mathrm{ }\to \mathrm{ }$ products?

For the zero order reaction, $\text{A}\to \text{B}+\text{C}$; initial concentration of A is 0.1 M. If [A] = 0.08 M after 10 minutes, then it's half life and completion time are respectively

Which of the following graph represents zero order reaction $\left[\mathrm{A}\left(\mathrm{g}\right)\to \mathrm{B}\left(\mathrm{g}\right)\right]$?

The unit and value of rate constant and that of rate of reaction are same for:

For zero-order reaction, the integrated rate equation will be:

The rate constant of a zero order reaction is $0.2 \mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }{\mathrm{d}\mathrm{m}}^{-3}\mathrm{ }{\mathrm{h}}^{-1}.$ If the concentration of the reactant after $30$min is$\mathrm{ }0.05\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }{\mathrm{d}\mathrm{m}}^{-3}.$ Then what would be its initial concentration?

The rate constant for a zero order reaction is:

The half-life period for a zero-order reaction $\mathrm{A}\to$$\mathrm{Product}$, is $100$ minutes. How long will it take for $80\%$ completion?

What is the integrated rate law for a zero order reaction?

The time required for 100% completion of a zero order reaction is

The plot between concentration versus time for a zero order reaction is represented by

For zero order reaction, the integrated rate equation is