Which is/are correct graph for given reactions?

Zero order reaction reaction:

$\left[\mathrm{A}\right]={\left[\mathrm{A}\right]}_{\circ }-\mathrm{kt}$

Comparing with equation of a straight line, y = mx + c, plot [A] against t, a straight line with slope = –k and intercept equal to [A]₀.

First order reaction reaction:

$\ln \left[\mathrm{A}\right]=\ln {\left[\mathrm{A}\right]}_{\circ }-\mathrm{kt}$

Comparing with equation of a straight line, y = mx + c, plot ln [A] against t, a straight line with slope = –k and intercept equal to ln [A]_0.

Half life of first order reactions can be written as follows.

$\begin{array}{l}{t}_{1/2}=\frac{0.693}{k}\end{array}$

This equation for the half life implies that the half life is independent temperature

Half life of second order reactions can be written as follows.

$\begin{array}{l}{t}_{1/2}=\frac{1}{k[R{]}_0}\end{array}$

This equation for the half life implies that the half life is inversely proportional to the concentration of the reactants.