All the catalyst remains as it is not incorporated into the reaction products, it just speeds up the reaction time.
The overall enthalpy change in a common reaction would not change. Only the path to get there would change. A catalyst basically lessens the activation energy required to get the reaction to take place.
The how much speed it takes for two substances to make one product. Many factors can affect this including the temperature, the surface area, the concentration, the catalyst and the pressure (only applies for gases)
Biocatalysts usually are very specific to the reaction that they catalyze. So many only speed up one reaction. Quite often a chain reaction occurs where numerous enzymes catalyze reactions at different points speeding up a process that would take much longer and propelling the reaction through numerous phases.
Zinc Chloride catalyses the reaction of e.g. phatalic anhydride and resorcinol. If you head these three as powdered substances with a bunsenburner, they react much faster. After solving this mixture in water, you can filtrate the Zinc Cholride out of the solution. For more examples what a catalyst does, read Wiki or Google catalyst. Good Luck
There are two ways in which catalysts work. You already know that when two different molecules bump into each other, they might react to make new chemicals. We usually talk about "collisions" between molecules, it would be much simpler to say that the molecules bumped into each other. How fast a chemical reaction is depends upon how frequently the molecules collide. You have probably been told about the "kinetic theory" which is all about heat and how fast molecules move around. What catalysts are doing when they make a chemical reaction go faster is to increase the chance of molecules colliding. The first method is by "adsorption", the second method is by the formation of intermediate compounds.Adsorption This occurs when a molecule sticks onto the surface of a catalyst. Make sure that you spell this word correctly; it is not the same as absorption. Here is an example: it is possible to use Platinum as a catalyst to make sulphur Trioxide from Sulphur Dioxide and Oxygen. Sulphur Trioxide is very important because it is used to make Sulphuric acid which is needed for car batteries. The molecules of the two gases (Sulphur Dioxide and Oxygen) get adsorbed (stuck onto) the surface of a Platinum catalyst. Because the two molecules are held so close together, it is more likely that they will collide and therefore react with each other. The Sulphur Trioxide easily falls off the catalyst leaving space for more Sulphur Trioxide and Oxygen.Intermediate Compounds Many catalysts, including all enzymes" work by forming intermediate compounds. What happens is very simple: the chemicals involved in the reaction combine with the catalyst making an intermediate compound, but this new compound is very unstable. When the intermediate compound breaks down it releases the new compounds and the original catalyst.
A lump of solid has a much lower surface area compared to a powdered catalyst. Since most chemical reactions that are catalysed by solid phase catalysts (heterogeneous catalysts) occur on the catalyst surface more surface area = faster reaction.
The term catalyst is much more general than the term hardener, since hardening is only one of endless numbers of processes which can be catalysed. A hardener, therefore, would be a specific type of catalyst.
When reactants are joined by a catalyst, they no longer have to collide with much energy to react. Thus, with the catalyst present the reaction can proceed at very low temperatures.
The presence of a catalyst affects the activation energy of a reaction by lowering the activation energy, helping the reaction go faster and making it so the reaction does not have to use as much energy to fulfill the products.
A catalyst by definition is not consumed in a reaction. Therefore, the mass remaining after a reaction will be equal to the mass before the reaction. Note that in certain reactions, such as free radical halogenation, the catalyst may be lost by certain side reactions, however.
The overall enthalpy change in a common reaction would not change. Only the path to get there would change. A catalyst basically lessens the activation energy required to get the reaction to take place.
its an iron catalyst (iron oxide)
The how much speed it takes for two substances to make one product. Many factors can affect this including the temperature, the surface area, the concentration, the catalyst and the pressure (only applies for gases)
Catalysts allow chemical changes to occur much more rapidly. Reactions that usually take years can happen before your eyes in seconds. From my understanding there is no 100% agreed upon reason for how they do this. There are a number of widely regarded theories though.
An enzyme catalyst will lower the amount of energy required to preform a reaction. This in turn, will make it much easier for the reaction to start. So yes, it will let a reaction reach equilibrium quicker. Other factors affecting the time of reaction are: The concentration of the reactants, (the less volume and more pressure you have will increase the rate of reaction) The PH level (especially important for biology reactions, protein enzymes are built for specific PH levels and will not work correctly if they are in another PH level, buffers can be used to stabilize pH levels)
The substrate fits into the enzyme, much the way a key fits in a lock. Sometimes there are other "modulators" that also fit in the enzyme.
It decreases the activation energy, or the energy barrier the reactants must go through to form products. This is the same thing as the energy of the transition state. By decreasing the activation energy necessary for the reaction to occur, more reactants are able to form products since not as much energy is needed. See the Web Links to the left of this answer for more information.