Hydrogen storage using activated carbons
Short answer: yes, if you want to store the same amount of hydrogen and on condition that you do not mess with pressure.

Long answer: I'll skip some intermediate physicochemical derivations for brevity. The phenomenon we are dealing with is called adsorption. Perhaps, the simplest theoretical explanation of adsorption was given by Langmuir. Langmuir adsorption isotherm can be written as $$\theta = \frac{Kp}{1 + Kp},$$ where $\theta$ is a fraction of the surface of adsorbent (solid) covered by the adsorbate (gas) and $K$ is an equilibrium constant. It is seen that at a constant temperature the more pressure you apply to the system, the more surface is covered (i.e. the more gas is adsorbed).

But what about the temperature dependence? Since $K$ is an equilibrium constant, its temperature dependence is defined by the van't Hoff equation. Also, $K$ is directly proportional to the pressure required for a certain amount of gas to be adsorbed. In other words, when $\theta$ is constant, $\ln{K}+\ln{p}=\mathrm{const}$, transforming our van't Hoff into something like $$\left(\frac{\partial\ln{p}}{\partial(1/T)}\right)_\theta=\frac{\Delta_{ad}H^○}{R}.$$ Here, $R$ is the gas constant, and the sign of $\Delta_{ad}H^○$ - adsorption enthalpy - is negative, for adsorption is exothermic. Consequently, the slope of $\ln{p}$ vs $1/T$ line is negative. In plain English, the equation above reads like this: in order to obtain the same amount of adsorbate $\theta$ you should either decrease the temperature or increase the pressure.

If you're that interested in the topic, you may also want to check out how the sorption pumps work.