The process, which is catalysed by one of the products, is called: (a) Acid base catalysis (b) Negative catalysis (c) Positive catalysis (d) Auto catalysis

Catalysis is a fundamental concept in chemistry that involves the acceleration of a chemical reaction by a substance called a catalyst. Unlike reactants, a catalyst isn't consumed in the reaction. It works by providing an alternative reaction pathway with a lower activation energy than the uncatalyzed reaction. A good analogy to understand this process is to think of a catalyst as a 'shortcut' in a maze – it doesn't change the start or end point, but it helps you get there faster.

Imagine you're trying to get paint to dry. On a humid day, it might take hours. If you add a substance that draws moisture out of the paint, it can dry much quicker. The substance isn't part of the final dried paint, but without it, the process would have taken much longer. That’s what catalysts do in chemical reactions; they speed things up without becoming part of the final product.

Catalysts come in various forms and can be classified based on how they interact in reactions. Firstly, there's heterogeneous catalysis, where the catalyst is in a different phase than the reactants, often seen in industrial processes. For example, solid catalysts are used to speed up reactions in liquid solutions.

In contrast, homogeneous catalysis occurs when the catalyst and the reactants are in the same phase. This can often be observed in the gas phase or within a single liquid solution.

Another fascinating type is enzyme catalysis, where biological molecules called enzymes act as highly efficient and specific catalysts for biochemical reactions. But the focus here is on auto catalysis, where one of the reaction products acts as a catalyst. As the reaction progresses, more of the product-catalyst is made, further speeding up the reaction. It's akin to having a snowball roll down a hill, growing larger and faster as it picks up more snow – an initial small amount of product speeds up its own production.

Chemical reactions are processes where reactants transform into products due to breaking and forming of chemical bonds. Picture this as a dance where partners (atoms or molecules) switch and form new pairs (products). To initiate this dance, energy is often needed, which is known as activation energy.

There are several types of chemical reactions such as synthesis, decomposition, single replacement, and double replacement. In the case of auto catalysis, we have a special scenario where the product of the reaction joins the dance floor and starts encouraging others to dance faster. The product facilitates the conditions that enable or accelerate more reactions to occur. This is a self-propagating reaction scenario, leading to even faster reaction rates as more product is formed, a beautiful example of chemistry in action.