Which of the following graphs would yield a straight-line plot?

With an increase in temperature, chemisorption initially rises before falling. The first rise is caused by the heat being delivered, which serves as activation energy. The exothermic nature of the adsorption equilibrium is what causes the subsequent decline.

$⟹\frac{\mathrm{x}}{\mathrm{m}}=\mathrm{k}\times (\mathrm{p}{)}^{\frac{1}{n}}$
where k and n are constants that depend on the nature of the adsorbent and the gas at a specific temperature, and x is the mass of the gas adsorbed on the mass m of the adsorbent under pressure P.

$⟹\log \left(\frac{\mathrm{x}}{\mathrm{m}}\right)=\log \left(\mathrm{k}\right)+\frac{1}{\mathrm{n}}\log \left(\mathrm{p}\right)$

When both sides of the equation are logarithmic,
The graph of logarithmic distribution using this equation and the usual equation of a straight line, $y=mx+c$