Is the effect of a catalyst dependent on its concentration?

Is the effect of a catalyst dependent on its concentration?

Sometimes a reaction depends on catalysts to proceed. In that case, changing the concentration of the catalyst can speed up or slow down the reaction. For example, enzymes speed up biological reactions, and their concentration affects the rate of reaction.

Why is ammonia decomposition zero order reaction?

In general, decomposition of a gas (like ammonia) on a metal surface (like platinum) is a zero order reaction. This is because the gas is adsorbed on the metal surface due to pressure and the initial concentration is immaterial.

How would you differentiate catalyst from temperature as a factor affecting the rate of reaction?

When the concentrations of the reactants are raised, the reaction proceeds more quickly. The reaction rate decreases with a decrease in temperature. Catalysts can lower the activation energy and increase the reaction rate without being consumed in the reaction.

How does catalyst affect the rate of reaction?

A catalyst is a substance that can be added to a reaction to increase the reaction rate without getting consumed in the process. Catalysts typically speed up a reaction by reducing the activation energy or changing the reaction mechanism.

Why does increasing the concentration of H2O2 increase the rate of decomposition?

In many living organisms hydrogen peroxide is a product of metabolism that must be broken down, since in appreciable concentrations it is toxic. The rate of decomposition is increased by the intra-cellular enzyme catalase.

Why does increasing the concentration increase the rate of reaction?

If the concentration of reactants is increased, there are more reactant particles moving together. There will be more collisions and so the reaction rate is increased. The higher the concentration of reactants, the faster the rate of a reaction will be.

Is decomposition of ammonia on platinum surface an example of first order reaction?

Answer: Decomposition of ammonia on the surface of platinum catalyst is zero order.

What is the order of reaction for decomposition of NH3 on platinum surface give reasons?

The decomposition of NH3 on platinum surface is zero order.

Why does the rate of most reactions increases with increasing temperature?

Increasing the temperature a reaction takes place at increases the rate of reaction. At higher temperatures, particles can collide more often and with more energy, which makes the reaction take place more quickly.

How does platinum catalyst work?

Platinum works as a catalyst by collecting oxygen atoms (O), and letting them bind with the toxic carbon monoxide (CO), to create the less harmful carbon dioxide (CO2). The researchers discovered that the oxygen atoms are somewhat “loose,” so that they can easily react with other substances.

Why does a catalyst cause a reaction to proceed faster?

The pathway involving the catalyst requires less activation energy and is therefore faster. A catalyst speeds up a chemical reaction, without being consumed by the reaction. It increases the reaction rate by lowering the activation energy for a reaction.

When the decomposition of ammonia is carried out on platinum surface?

When the decomposition of ammonia is carried out on platinum surface at 1000°C the hydrogen binds strongly on the surface. Prove the that the rate is equal to d p ( N H 3) d t = − k p ( N H 3) p ( H 2).

What is the effect of θn on ammonia decomposition reaction?

Here, a high value for θN (high coverage of N (ad)) will promote the forward reaction in reaction step (V), that is, formation of N 2 (ad) from one strongly adsorbed and one weakly adsorbed nitrogen atom, thus 2 N (ad), and thus the overall ammonia decomposition reaction, 16 and vice versa.

Why is it not possible to completely decompose ammonia into hydrogen?

Thus, decomposition of ammonia to hydrogen (and nitrogen) requires an energy input, and since the decomposition reaction is very slow even at relatively high temperatures, a catalyst is also needed. Since the reaction is an equilibrium reaction, it is not possible to completely decompose ammonia into hydrogen.

Is it easier to study ammonia synthesis or decomposition?

It is much easier to study ammonia decomposition than ammonia synthesis since the decomposition reaction, when carried out at reasonably high temperatures, can be considered to be essentially irreversible. Further, it need not be studied under high pressure and so the interpretation of kinetic measurements is much more straightforward.