A certain zero order reaction has $\mathrm{k}=0.025\mathrm{ }\mathrm{M}\mathrm{ }{\mathrm{s}\mathrm{e}\mathrm{c}}^{-1}$ for the disappearance of $\mathrm{A}$. What will be the concentration of $\mathrm{A}$after $15$seconds if initial concentration is $0.5 \mathrm{M}$.

A graph plotted between $\log {\mathfrak{t}}_{50\%} \mathrm{vs}$. $\log$  concentration is a straight line. What conclusion can you draw from this graph?

What will be the order of reaction and rate constant for a chemical change having $\log {\mathrm{t}}_{50\%} \mathrm{vs} \log$ a concentration of $\left(\mathrm{A}\right)$(A) curves as:

Which integrated equation is correct for the following ${\mathrm{I}}^{\mathrm{st}}$ order reaction started with only $\mathrm{A}\left(\mathrm{g}\right)$ in a closed rigid vesset.

$\mathrm{A}\left(\mathrm{g}\right)⟶\mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$

${\mathrm{P}}_{\mathrm{i}}=$ initial pressure; ${\mathrm{P}}_{\mathrm{t}}=$total pressure at time $\mathrm{t}$