Why can sulfur act like a catalyst?
It's not a catalyst here. It speeds up the reaction, which is why it acts like a catalyst.

Here is the reaction without sulfur:

$\ce{6 KNO3 + C7H8O -&gt; 3 K2CO3 + 4 CO2 + 2 H2O + 3 N2}$

And here it is with sulfur:

$\ce{4 KNO3 + C7H4O + 2 S —&gt; 2 K2S + 4 CO2 + 3 CO + 2 H2O + 2 N2}$

(Source)

Sulfur decreases the ignition temperature, as well as probably contributing a bit to the rate. Here, it is effectively turning $\ce{CO2}$ and $\ce{K2CO3}$ to $\ce{CO}$ and $\ce{K2S}$. If you take into account Le Chatelier's principle, the conversion of the products of the basic reactants speeds it up. (The decrease in concentrations/activities of the products due to their conversion means that the equilibrium shifts in the forward direction to compensate for it.)

So it is speeding up the reaction and making it easier to carry out. Not a catalyst.

A note: There's no reason why any element/compound can't act as a catalyst. Transition metals are generally catalysts in a certain type of reaction, and they generally catalyze the reaction by adsorbing the gases. Catalysts can work in many other ways—generally, they form intermediates in the reaction and present an alternative path via the intermediate. ($\ce{V2O5}$, for example, is a catalyst in many reactions involving organic compounds since it forms cyclic intermediates with various groups).